Methane and hydrogen sulfide react to form hydrogen and carbon disulfide, like this: CH₂(g) + 2H₂S(g) → 4H₂(g)+cS₂(g) Use this chemical equation to answer the questions in the table below. Suppose 210. mmol of CH4 and 420. mmol of H₂S are added to an empty flask. How much CH will be in the flask at equilibrium? Suppose 115. mmol of H₂ and 28.8 mmol of CS, are added to an empty flask. How much CH will be in the flask at equilibrium? None. O Some, but less than 210. mmol. ○ 210. mmol. O More than 210. mmol. O None. Some, but less than 28.8 mmol. 28.8 mmol. More than 28.8 mmol.

Methane and hydrogen sulfide react to form hydrogen and carbon disulfide, like this: CH₂(g) + 2H₂S(g) → 4H₂(g)+cS₂(g) Use this chemical equation to answer the questions in the table below. Suppose 210. mmol of CH4 and 420. mmol of H₂S are added to an empty flask. How much CH will be in the flask at equilibrium? Suppose 115. mmol of H₂ and 28.8 mmol of CS, are added to an empty flask. How much CH will be in the flask at equilibrium? None. O Some, but less than 210. mmol. ○ 210. mmol. O More than 210. mmol. O None. Some, but less than 28.8 mmol. 28.8 mmol. More than 28.8 mmol.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Chapter 1 question 10
Hydrogen and iodine react to form hydrogen iodide, like this: H₂(g) + I₂(g) → 2 HI(g) Use this chemical equation to answer the questions in the table below. Suppose 220. mmol of H₂ and 220. mmol of I₂ are added to an empty flask. How much HI will be in the flask at equilibrium? Suppose 175. mmol of HI are added to an empty flask. How much HI will be in the flask at equilibrium? None. Some, but less than 440. mmol. 440. mmol. More than 440. mmol. None. Some, but less than 175. mmol. O 175. mmol. More than 175. mmol. X Ś
Consider the following reaction: 2 NH3(g) 2 3 H2(g) + N2(g) Kc = 2.20 1.10 mol/L of nitrogen gas, 0.50 mol/L of hydrogen gas, and 0.25 mol/L of ammonia gas are added to an empty flask. Which way, if at all, will the reaction shift to reach equilibrium? The reaction will shift left to make more reactants and reach equilibrium. The reaction is already at equilibrium and, therefore, will not shift in either direction. The reaction will shift left to make more products and reach equilibrium. O The reaction will shift right to make more products and reach equilibrium. The reaction will shift right to make more reactants and reach equilibrium.
For the chemical equation: SO2(g) + NO2(g) SO3(g) + NO(g) The equilibrium constant at a certain temperature is 8.80. At this temperature, calculate the number of moles of NO2(g) that must be added to 6.20 mol SO2(g) in order to form 4.40 mol SO3(g) at equilibrium.
The chemical equation represents a reaction at equilibrium. 2SO3(g) = 2SO2 (g) +O2(g) Which of these shows the equilibrium constant expression for this chemical equation? A [O2][SO2]2/[SO3]2 B [O2]2[SO2]/2[SO3] C 2[SO3]/[O2]2[SO2] D [SO3]2/[O2][SO2]2
Consider the combustion of methane (as represented by the following equation). This is the reaction that occurs for a Bunsen burner, which is a source of heat for chemical reactions in the laboratory. CH 4(9) +20 2(g) =CO2(g) + 2H 20(g) For the system at chemical equilibrium, which of the following explains what happens if the temperature is reduced? O a. The equilibrium position is shifted to the left and the value for K increases. O b. The equilibrium position is shifted to the right and the value for K increases. O c. The equilibrium position is shifted to the right and the value for K decreases. O d. The equilibrium position is shifted but the value for K stays constant. Oe. The equilibrium position is shifted to the left and the value for K decreases.
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Which of the following occurs when reactants are removed from a chemical reaction in solution or the gas phase at equilibrium? * O Product increases, so the equilibrium shifts to produce more products. O Reactant increases, so the equilibrium shifts to produce more products. O Reactants decreases, so the equilibrium shifts to produce more reactants. O Product decreases, so the equilibrium shifts to produce more reactants. The reaction [20 CO2 + 22 H:O → 2 Cz0H22 + 31 O:], in general terms, is: Reversible O Irreversible The reaction [N:O: = 2 NO: ], in general terms, is: * Reversible Irreversible
Consider the following reaction at equilibrium. What effect will removing some SO2 have on the system? SO2(g) + NO2(g) = SO3(g) + NO(g) The pressure of SO3 will increase The equilibrium constant will decrease. No change will occur since SO2 is not included in the equilibrium expression. The pressure of NO2 will increase. The reaction will shift to decrease the pressure.
1.QuestionGiven the reaction at equilibrium: 2 SO2(g) + O2(g) <--> 2 SO3(g) + heat Which change will shift the equilibrium to the right? increasing the temperature increasing the pressure decreasing the amount of SO2(g) decreasing the amount of O2(g)
What does it mean for a chemical reaction to reach equilibrium? The rates of the forward and reverse reactions are equal. The concentrations of the reactants and products are also equal. The rates of the forward and reverse reactions are increasing. The concentrations of the reactants and products are equal. The rates of the forward and reverse reactions are equal. The concentrations of the reactants and products are constant. The rates of the forward and reverse reactions are increasing. The concentrations of the reactants and products are also increasing.
Chapter 1 question 1