1. Consider the reaction below. N2(g) + 3 H2(g) ⇋ 2 NH3(g) Which of the following changes would cause less NH3 to be produced?
decreasing the volume |
adding N2 |
increasing the volume |
adding H2 |
2. Consider the following reaction. N2(g) + 3 H2(g) ⇋ 2 NH3(g) The forward reaction is exothermic. Which of the following changes would cause less NH3 to be produced?
decreasing the temperature | |
adding H2 | |
increasing the temperature | |
adding N2 3. What is the effect of a catalyst on a reaction? Drag the terms on the left to the appropriate blanks on the right to complete the sentences.
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4. Why are catalysts so important to chemistry?
Catalysts are important in chemistry because they make reactions to be exothermic. | ||||
Catalysts are important in chemistry because they help to measure the temperature of the reaction. | ||||
Catalysts are important in chemistry because many reactions would be too slow to be useful without catalysts. | ||||
Catalysts are important in chemistry because they help to calculate the masses of reactants.. 5. Enzymes work in biological systems by _________.
pLEASE help! No need an explanation!..thanks |
1. Consider the reaction below. N2(g) + 3 H2(g) ⇋ 2 NH3(g) Which of the following...
QUESTION 2 Consider the following reversible reaction at equilibrium: 3H2(g) + N2(g) → 2NH3(g) + heat Which of the following changes will shift the equilibrium towards the products (right side)? Decreasing the amount of NH3. Increasing the temperature. Adding a catalyst to the system. Decreasing the amount of H2. Increasing the volume of the system.
For the exothermic reaction 3H2(g) + N2(g) ↔ 2NH3(g) + HEAT, which of the following changes could be carried out to cause the reaction to shift to the right? Adding H2 Adding NH3 Increasing the temperature Removing N2
Consider the following system at equilibrium. N2(g) + 3 H2 (g) 2 NH3(g) + 92.24 kJ <--> Which response includes all of the following that will shift the equilibriu to the right, and no others? I. increasing the temperature III. increasing the pressure II. decreasing the temperature IV. decreasing the pressure VI. adding some NH3 V. removing some NH3 VII. removing some N2 VIII. adding some N2 a) I, IV, VI, and VII c) I, VI, and VII e) II,...
Consider the reaction: 2 NH3 (g) → 3 H2 (g) + N2 (g) Which of the following is true about entropy associated with this reaction? A. The entropy of the system will be positive because the mol of gas is increasing. B. The entropy of the system will be negative because the mol of gas is decreasing. C. The entropy of the system will be negative because the mol of gas is increasing. D. The entropy of the system will...
1. For the following reaction N2 (g) + 3 H2(g) — 2 NH3(g) AH° = -92.4 kJ K = 1.245 x 10-5 at 427°C for each change listed, predict the equilibrium shift and the effect on the indicated quantity. Direction of Shift Gt; or no change) Effect on Quantity Change Effect (increase, decrease, or no change) amount of NH3(g) amount of N2(g) (a) decrease in volume (b) Decrease temperature (c) addition of H2(g) (d) addition of NH3(g) (e) removal of...
Consider the reaction: N2(g) + 3 H2(g) « 2 NH3(g) a. Write the expression for the equilibrium constant, K, for this reaction. b. An equilibrium misture of N2, H2, and NH3 at 300°C is analyzed, and it is found that: [N2] = 0.25 mol/L, [H2] = 0.15 mo/L, and [NH3] = 0.090 mol/L. Find K at 300°C for this reaction.
QUESTION 1 Consider the following chemical reaction: Mg(s) + 2HCl(aq) – MgCl2(aq) + H2(g) Which of the following changes will decrease the rate of this reaction? Adding more solid Mg. Adding a catalyst. Decreasing the pressure of H2. Decreasing the temperature. Increasing the concentration of HCI.
QUESTION 1 Consider the following chemical reaction: Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g) Which of the following changes will decrease the rate of this reaction? Adding more solid Mg. Adding a catalyst. Decreasing the pressure of H2. Decreasing the temperature. Increasing the concentration of HCI.
You are running the synthesis of ammonia reaction: 3 H2(g) + N2(g) --> 2 NH3(g) You add 15 g N2 and 9.0 g H2 to your reaction flask. Which of the following statements are true? (More than one option may be correct) H2 is the limiting reactant because the limiting reactant calculation showed that less NH3 can be produced from H2 as compared to the amount of NH3 possible from the N2. N2 is the limiting reactant because the limiting...
Consider the reaction H2(g) + Cl2(g) ⇌ 2HCl(g) which of the following stresses will cause the reaction shift in the forward direction? a. decreasing the pressure b. removing some HCl(g) c. increasing the pressure d. removing some H2(g) Consider the reaction N2(g)+2O2(g)→2NO2(g), which stress will cause the reaction shift to the left a. increasing the pressure b. removing some NO2(g) c. adding a catalyst d. decreasing the pressure Phenolphthalein is an indicator with a pH range from 8.3 to 10.0....