The following reaction occurred at a constant rate of 0.00130 M/s in a container with a volume of 0.650 L. A(g) + B(g) → 2 C(g) How many moles of C are produced after 6.72 s? Select one: O 0.0148 mol O 0.0114 mol O 0.00284 mol O 0.00568 mol
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- Determine rxnH 25 C for the following reaction: NO g O2 g NO2 g This reaction is a major participant in the formation of smog.10.0 moles of N2O were placed in a 2.00-L container at a given temperature where it decomposes according to:N2O(g) ------------> N2(g) + O2(g) At eq., 2.20 moles of N2O remain. Calculate the value of Kc for the reaction.Calcium oxide (CaO), an important ingredient in cement, is produced by decomposing calcium carbonate (CaCO3) at high temperature: CaCO3(s) → CaO(s) + CO2(g) In one particular reaction, 70 g of CaCO3 is heated at 450°C in a 5.0 L vessel. The pressure of CO2 is 0.24 atm after 4.0 minutes. What is the average rate of CO2 production in moles per minute during the 4 minutes? (Enter in mol/min.) If you assume this rate of decomposition remains constant, how many minutes will it take for the entire sample of CaCO3 to decompose?
- A flask is charged with 0.120 mol of A and allowed to react to form B according to the following hypothetical gas-phase reaction. A(g) -> B(g) The following data are collected. times (s) 0 40 80 120 160 moles of A 0.120 0.063 0.046 0.026 0.015 (a) Calculate the number of moles of B at each time in the table.0 s ___mol40 s ___mol80 s ___mol120 s ___mol160 s ___mol(b) Calculate the average rate of disappearance of A for each 40 s interval, in units of mol/s.0 - 40 s ___mol/s40 - 80 s ___mol/s80 - 120 s___ mol/s120 - 160 mol/s ___mol/sA researcher fills an evacuated 1.5L flask with 2.5 mols of N2O5 gas and allows the reaction to proceed at 350oC. At equlibrium [N2O5] = 0.20M, calculate Kc. Write answer in decimal form to four significant figures.QUESTION 10 Measurements taken during the following reaction showed a concentration of carbon monoxide (CO) of 196.9 mol/L at 13.9 min and of 122.7 mol/L at 29.5 min. CO (g) + NO2 (g) --> CO2 (g) + NO (g) Calculate the average rate of the gain of carbon dioxide (CO2) in M/sec. Write the answer in scientific notation with 3 sig.dig.
- Calcium oxide, an important ingredient in cement, is produced by decomposing calcium carbonate at high temperature: CaCO3(s) → CaO(s) + CO2(g) In one reaction, 3.9 kg of calcium carbonate is heated at 589 °C in a 20.0-L vessel. The pressure of CO2 is 0.18 bar after 6.5 minutes. question 1. What is the average rate of CO2 production in mol/min during the 6.5-minute interval? question 2. How many moles of calcium carbonate consumed in the 6.5-minute interval?The reform reaction between steam and gaseous methane (CH4) produces "synthesis gas," a mixture of carbon monoxide gas and dihydrogen gas. Synthesis gas is one of the most widely used industrial chemicals, and is the major industrial source of hydrogen. Suppose a chemical engineer studying a new catalyst for the reform reaction finds that 178. liters per second of methane are consumed when the reaction is run at 189.°C and the methane is supplied at 0.51atm. Calculate the rate at which dihydrogen is being produced. Give your answer in kilograms per second. Round your answer to 2 significant digits. =___kg/sA reaction at 8.0°C evolves 211.mmol of carbon dioxide gas. Calculate the volume of carbon dioxide gas that is collected. You can assume the pressure in the room is exactly 1 atm. Round your answer to 3 significant digits.
- One reaction that occures in an automobile catalytic converter is the conversion of nitrogen monoxide to nitrogen and oxygen. 2NO(g) --> N2(g) + O2(g) A) write the relative rates of consumption and formation using the balanced equation. B) If the rate is 0.250 M/s over the first 5.50 s, how much NO(g) will be consumed?Nitric Oxide, NO , reacts with hydrogen to give nitrous oxide, N2O, and water. 2NO(g) +H2(g) → N2O(g) + H2O(g) In a series of experiments, the following initial rates of disappearance of NO were obtained: Expriment Initial Conc. of NO Initial Conc. of H2 Initial Rate Exp. 1 6.4x10-3 M 2.2x10-3 M 2.6x10-5 M/s Exp. 2 12.8x10-3 M 2.2x10-3 M 1.0x10-4 M/s Exp. 3 6.4x10-3 M 4.5x10-3 M 5.1x10-5 M/s What is the value of the rate constant for the reaction? Express your answer to three significant figures. Just enter the number (e.g. 2.48x10^-4) and the unit.Nitric Oxide, NO , reacts with hydrogen to give nitrous oxide, N2O, and water. 2NO(g) +H2(g) → N2O(g) + H2O(g) In a series of experiments, the following initial rates of disappearance of NO were obtained: Expriment Initial Conc. of NO Initial Conc. of H2 Initial Rate Exp. 1 6.4x10-3 M 2.2x10-3 M 2.6x10-5 M/s Exp. 2 12.8x10-3 M 2.2x10-3 M 1.0x10-4 M/s Exp. 3 6.4x10-3 M 4.5x10-3 M 5.1x10-5 M/s What is the rate law for the reaction? Input the answer in the form rate = k[A]2[B]