(BASIC QUESTIONS) Choose or tick the phase of matter that is being described CHOICES: GAS LIQUID EITHER NEITHER Highest kinetic energy among its molecules Has a definite mass
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(BASIC QUESTIONS) Choose or tick the phase of matter that is being described
CHOICES:
- GAS
- LIQUID
- EITHER
- NEITHER
- Highest kinetic energy among its molecules
- Has a definite mass
- Molecules are tightly packed in an organized manner
- Follows the shape of its container
- Molecules move in random motion
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- You have two distinct gaseous compounds made from element X and element Y. The mass percents are as follows: Compound I: 30.43% X, 69.57% Y Compound II: 63.64% X, 36.36% Y In their natural standard states, element X and element Y exist as gases. (Monatomic? Diatomic? Triatomic? That is for you to determine.) When you react gas X with gas Y to make the products, you get the following data (all at the same pressure and temperature): 1 volume gas X + 2 volumes gas Y 2 volumes compound I 2 volumes gas X + 1 volume gas Y 2 volumes compound II Assume the simplest possible formulas for reactants and products in the chemical equations above. Then, determine the relative atomic masses of element X and element Y.You have two distinct gaseous compounds made from element X and element Y. The mass percents are as follows: Compound I: 30.43% X, 69.57% Y Compound II: 63.64% X, 36.36% Y In their natural standard states, element X and element Y exist as gases. (Monatomic? Diatomic? Triatomic? That is for you to determine.) When you react gas X with gas Y to make the products, you get the following data (all at the same pressure and temperature): 1. volume gas X + 2 volumes gas Y2 volumes compound I 2. volumes gas X + 1 volume gas Y2 volumes compound II Assume the simplest possible formulas for reactants and products in the chemical equations above. Then, determine the relative atomic masses of element X and element Y.Suppose that you are closing a cabin in the north woods for the winter and you do not want the water in the toilet tank to freeze. You know that the temperature might get as low as 30. C, and you want to protect about 4.0 L water in the toilet tank from freezing. Calculate the volume of ethylene glycol (density = 1.113 g/mL; molar mass = 62.1 g/mol) you should add to the 4.0 L water.
- 5.127 Photosynthesis produces glucose (C6H12O6) and oxygen from carbon dioxide and water:If limestone is interacted with an acid, it liberates a gas made from: a. water vapor b. methane c. oxygen d. carbon dioxide *This is a multiple choice type of questionYou have two distinct gaseous compounds made from element X and element Y.The mass percents are as follows: Compound I: 30.43% X, 69.57% Y Compound II: 63.64% X, 36.36% Y In their natural standard states, element X and element Y exist as gases. (Monatomic? Diatomic? Triatomic? That is for you to determine.) When you react "gas X" with "gas Y" to make the products, you get the following data (all at the same pressure and temperature): 1 volume "gas X" + 2 volumes "gas Y" → 2 volumes compound I 2 volumes "gas X" + 1 volume "gas Y" → 2 volumes compound II Assume the simplest possible formulas for reactants and products in the chemical equations above. Then, determine the relative atomic masses of element X and element Y.
- The U.S. proven natural gas reserves in 2013 were 323 trillion ft3 . How long will these reserves last if there are no imports or exports and if the U.S. annual rate of use of 24.5 trillion ft3 continues?The mystery fuel speedster! (Homework ) For fun, you build an explosive car with your little brother by attaching wheels to an empty windshield washer container. To advance it, you add 1.20 ml ( = 0.7915 g/ml) of a liquid but volatile fuel into the container. You close the cap and shake to evaporate the liquid. Finally, you place the car on its wheels, remove the cap and insert a burning wooden rod into the container. A flame suddenly comes out of the car, which is propelled with good speed in front of your little brother surprised, but all upset by the maneuver. The volatile fuel is composed of 37.5% carbon, 12.6% hydrogen and 49.9% oxygen. Its molar mass is approximately 32.0 g/mol. During the reaction, the fuel (gaseous) burns in the presence of gaseous oxygen, and the products of the reaction are carbon dioxide and water, gaseous too. The volume of the windshield washer container used is 4.00 litres. Useful Info: There is 21.0% gaseous oxygen in the air and initial conditions…Nitroglycerin is a dangerous powerful explosive that violently decomposes when it is shaken or dropped. The Swedish chemist Alfred Nobel (1833-1896) founded the Nobel Prizes with a fortune he made by inventing dynamite, a mixture of nitroglycerin and inert ingredients that was safe to handle. A.) Write a balanced chemical equation, including physical state symbols, for the decomposition of liquid nitroglycerin ( C3H5(NO3)3 ) into gaseous dinitrogen, gaseous dioxygen, gaseous water and gaseous carbon dioxide. B.) Suppose 79.0L of carbon dioxide gas are produced by this reaction, at a temperature of −8.0°C and pressure of exactly 1 atm . Calculate the mass of nitroglycerin that must have reacted in grams. Round your answer to 3 significant digits
- Although we tend to make less use of mercury these days because of the environmental problems created by its improper disposal, mercury is still an important metal because of its unusual property of existing as a liquid at room temperature. One process by which mercury is produced industrially is through the heating of its common ore cinnabar (mercuric sulfide, HgS) with lime (calcium oxide, CaO). 4 HgS(s) + 4 CaO(s) → 4 Hg(l) + 3 CaS(s) + CaSO4(s) What mass of mercury would be produced by complete reaction of 10.7 kg of HgS? kgCombustion of hydrocarbons such as undecane (C11H24) produces carbon dioxide, a "greenhouse gas." Greenhouse gases in the Earth's atmosphere can trap the Sun's heat, raising the average temperature of the Earth. For this reason there has been a great deal of international discussion about whether to regulate the production of carbon dioxide. 1. Write a balanced chemical equation, including physical state symbols, for the combustion of liquid undecane into gaseous carbon dioxide and gaseous water. 2. Suppose 0.310kg of undecane are burned in air at a pressure of exactly 1atm and a temperature of 18.0°C. Calculate the volume of carbon dioxide gas that is produced. Round your answer to 3 significant digits. = LCalculate the number of Argon atoms necessary to exactly cover a “metric” football field witha layer of Argon atoms that is one atom thick. Assume the football field is 100.0 m long and 50.0 m wide. Assume the kinetic diameter of an Argon atom is 3.4 Å and is to be taken as the actual diameter of the atom, d. Assume that the Argon atoms are all touching each other at their edges so that the center of each atom is 3.4 Å away from the next closest atom. (1.000 Å = 1.000x10-10m)