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Concept explainers
(a)
Interpretation: This is to determine whether the given statement for the number of molecules of oxygen and hydrogen gases present in two separate flasks under the given conditions is true of false.
Concept introduction:
Pressure, volume, temperature and number of moles of a gas are related through a
(b)
Interpretation: This is to determine whether the given statement for the pressure of oxygen and hydrogen gas present in two separate flasks under the given conditions is true of false.
Concept introduction:
Ideal gas equation is represented as follows:
Here, P is pressure, V is volume, n is number of moles, R is Universal gas constant and T is temperature.
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Chapter 11 Solutions
EBK BASIC CHEMISTRY
- (6.6: Similar to For practice 6.10) The mixture of gas contains 3.5 g Ne and 2.5 g He. What is the total pressure be for the partial pressure of Ne to be 0.25 atm? O 1.5 atm O 0.43 atm O 2.1 atm O 1.2 atmarrow_forward4.00 mol CO₂ is placed in a 6.00 L container at a temperature where 12.3% of it decomposes. What is the value of Kc for the following at this temperature? 2 CO₂(g) = 2 CO(g) + O₂(g) X Kc = 4.0✔ 4.76e-4arrow_forward320 29. Determine what happens to each variable below (increases, decreases, no change) under the stated conditions. Assume that all other variables not specifically mentioned are constant values. (10.4) (a) What happens to the pressure when the volume decreases? (b) What happens to the volume when the temperature increases? (c) What happens to the pressure when the temperature decreases? (d) What happens to the pressure when the amount of gas decreases? 30. Determine what happens to each variable below (increases, decreases, no change) under the stated conditions. Assume that all other variables not specifically mentioned are constant values. (10.4) (a) What happens to the volume if the amount of gas doubles? (b) What happens to the temperature when the pressure decreases? (c) What happens to the temperature when the volume increases? 34. Calculate the missing variables in each experiment below using Boyle's law. (10.5) (a) P, = 1.67 atm, V1 = 3.77 L, P2 = 0.229 atm, V2 = ? (b) P1 =…arrow_forward
- (7.50ml) Charles' Law 1. Several balloons are inflated with helium to a volume of 0.75 L at 27°C. One of the balloons was found several hours later, the temperature had dropped to 22°C. What would be the volume of the balloon when found, if no helium has escaped? (0.74L) Sign out V 8 12 DELL %23 %24 & 4 6 [O e r t y u d. f m alt ctri ofarrow_forward4.00 mol CO2 is placed in a 6.00 L container at a temperature where 12.3% of it decomposes. What is the value of Kc for the following at this temperature? CO2(g) 2 CO(g) + O2(g)arrow_forward: Three identical flasks contain three different gases at standard temperature and pressure. Flask A contains CH4 flask B contains O3, and flask C contains N2. Which flask contains the largest number of molecules?arrow_forward
- Automobile air bags employ a chemical reaction involving the rapid decomposition of sodium azide (NaN3) into sodium metal and nitrogen gas to inflate in a collision. How much sodium azide is required to decompose to inflate a 20.0 L air bag? Assume that the gas is at standard temperature and pressure, and thus occupies 22.4 L per mole. (AW: Na=23; N=14.007)arrow_forward(6.3: Avogadro's Law, Similar to Question 38 on page 256) A cylinder with a moveable piston contains 0.200 mol of gas and has a volume of 125 mL. What is its volume (in mL) if an additional 0.200 mol of gas is added to the cylinder. Assume constant pressure and temperature. O 500 mL O 62.5 mL O 250 ml. 125 mlarrow_forward27. 1.20 g of a gas compound containing C, H and S in 2.10 L. flask has the pressure of 108 mmHg at the temperature of 25oC . 1.00 g of the compound is burned in pure oxygen produces 2.24 g CO2 and 0.551 g H2O. 0.480 g of the compound produces 0.313 g SO2. Calculate the molecular formula of the compound. C = 12.01 g/mole , H = 1.00 g/mole, S = 32.07 g/mole, O = 16.00 g/mole Group of answer choices a.CH3S b.CHS c.C2H3S2 d.C5H6Sarrow_forward
- If 88.0 grams of carbonic acid are sealed in a 2.00 L soda bottle at room temperature (298.15 K) and decompose completely via the equation below, what would be the final pressure of carbon dioxide (in atm) assuming it had the full 2.00 L in which to expand? H:CO:(aq) H:0(1) + CO:(g) 4 7. +/-arrow_forward27. 1.20 g of a gas compound containing C, H and S in 2.10 L. flask has the pressure of 108 mmHg at the temperature of 25oC . 1.00 g of the compound is burned in pure oxygen produces 2.24 g CO2 and 0.551 g H2O. 0.480 g of the compound produces 0.313 g SO2. Calculate the molecular formula of the compound. C = 12.01 g/mole , H = 1.00 g/mole, S = 32.07 g/mole, O = 16.00 g/mole a.C2H3S2b.C5H6Sc.CH3Sd.CHSarrow_forward27. 1.20 g of a gas compound containing C, H and S in 2.10 L. flask has the pressure of 108 mmHg at the temperature of 25oC . 1.00 g of the compound is burned in pure oxygen produces 2.24 g CO2 and 0.551 g H2O. 0.480 g of the compound produces 0.313 g SO2. Calculate the molecular formula of the compound. C = 12.01 g/mole , H = 1.00 g/mole, S = 32.07 g/mole, O = 16.00 g/mole a.CH3S b.CHS c.C2H3S2 d.C5H6Sarrow_forward
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