---**Equilibrium Partial Pressure Calculation**For the reaction:\[ K_p = 0.032 \, \text{for the reaction} \]\[ \text{N}_2(g) + 3\text{H}_2(g) \rightleftharpoons 2\text{NH}_3(g) \]at a certain temperature. Suppose it was found that in an equilibrium mixture of these gases the partial pressure of \(\text{NH}_3(g)\) is 16.3 atm and the partial pressure of \(\text{N}_2\) is 4.82 atm. **Problem:**What is the partial pressure of \(\text{H}_2(g)\)?**Solution:**Enter your answer:The partial pressure of \(\text{H}_2(g)\) = \(\boxed{\text{?}}\) atm---**Note:** In this context, you'll use the equilibrium constant formula involving partial pressures to solve for the unknown.

Answered: Image /qna-images/answer/b9711bf9-8ca1-4a0a-be57-839b8e8e3e07.jpg

Kp = 0.032 for the reaction N₂(g) + 3H₂(g) → 2NH3(g) at a certain temperature. Suppose it was found that in an equilibrium mixture of these gases the partial pressure of NH3(g) is 16.3 atm and the partial pressure of N₂ is 4.82 atm. What is the partial pressure of H₂(g)? The partial pressure of H₂(g) = i ! atm

Kp = 0.032 for the reaction N₂(g) + 3H₂(g) → 2NH3(g) at a certain temperature. Suppose it was found that in an equilibrium mixture of these gases the partial pressure of NH3(g) is 16.3 atm and the partial pressure of N₂ is 4.82 atm. What is the partial pressure of H₂(g)? The partial pressure of H₂(g) = i ! atm

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...

See similar textbooks

Similar questions

Consider the synthesis of ammonia: N2(g) + 3H2(g)<=>2NH3(g) At 926.5 °C, the equilibrium constant Kp is 4.09 × 10–5. What is the value of Kc?
Consider the reaction N2(g) + O2(g) = 2NO(g) If the equilibrium partial pressures of N2, O2, and NO are 0.28, 0.26, and 0.025 atm, respectively, at 2200°C, what is Kp?
For the reaction CCl4(g) = C(s) + 2Cl₂(g) Kp = 0.76 at 700 °C. What initial pressure of pure carbon tetrachloride will produce a TOTAL equilibrium pressure of 2.80 atm at 700 °C?
A student ran the following reaction in the laboratory at 295 K:2NO(g) + Br2(g) 2NOBr(g)When she introduced NO(g) and Br2(g) into a 1.00 L evacuated container, so that the initial partial pressure of NO was 1.26 atm and the initial partial pressure of Br2 was 0.587 atm, she found that the equilibrium partial pressure of NOBr was 0.701 atm.Calculate the equilibrium constant, Kp, she obtained for this reaction.Kp =
R Manipulating Equilibrium Constant Expressions equilibrium constant for the following reaction is 63.3 at 378 °C. K 63.3 at 378 °C H₂(g) + 12(g) = 2 HI(g) culate the equilibrium constant for the following reactions at 378 °C. a) 2 HI(g) = H₂(g) + I2(g) K = (b) HI(g) 1/2 H₂(g) + 1/2 I2(g) Show Approach Show Tutor Steps Submit Submit Answer Try Another Version K = [References] 4 item attempts remaining Previous Next
For the reaction PCL5 (g) = PCl3 (g) + Cl₂ (g) at equilibrium, Kp = 321. The equilibrium partial pressures of PCl3 and Cl₂ are 1.00E0 atm and 4.50E0 atm, respectively. What is the equilibrium partial pressure of PCl5?
The reaction C(s) + 2 H₂(g) = CH₂(g) has Kp = 0.263 at 1000. K. Calculate the total pressure at equilibrium when 4.305 g of H₂ and 22.06 g of C(s) are placed in a 9.08 L flask and heated to 1000. K. Ptotal = Calculate the total pressure when 4.305 g of H₂ and 7.404 g of C(s) are placed in a 9.08 L flask and heated to 1000. K. Ptotal = atm atm
Consider the equilibrium system described by the chemical reaction below. If the partial pressures at equilibrium of NO, Cl2, and NOCI are 0.095 atm, 0.171 atm, and 0.28 atm, respectively, in a reaction vessel of 7.00 L at 500 K, what is the value of Kp for this reaction? 2 NO(g) + Cl2(g) = 2 NOCI(g)
Nitric oxide is formed in automobile exhaust when nitrogen and oxygen in air react at high temperatures, according to the following reaction. N2(g) + O2(g) ⇌ 2 NO(g) The equilibrium constant for the reaction is KP = 0.233 at 1840 ℃. If a container is charged with 0.403 atm of nitrogen and 0.300 atm of oxygen and the mixture is allowed to reach equilibrium, what will be the equilibrium partial pressure of nitrogen? Report your answer to THREE significant figures.
For the equilibrium N2O4(g) <----> 2 NO2(g), at 298 K, Kp = 0.15. For this reaction system, it is found that the partial pressure of N2O4 is 3.7 × 10^–2 atm at equilibrium. What is the partial pressure of NO2 at equilibrium?
3. Consider the reaction Br2 (g) + Cl2 (g) 2 BrCl (g) Kp = 1.11 x 104 at 150 K. A reaction mixture initially contains a Br2 partial pressure of 0.993 atm and a Cl2 partial pressure of 0.967 atm at 150 K. Calculate the equilibrium partial pressure of each reactant and product. 4. Consider the reaction CO₂ (g) + H2 (g) A reaction mixture initially contains a CO partial pressure of 1.768 atm and a H₂O partial pressure of 2.324 atm at 2000 K. Calculate the equilibrium partial pressures of each reactant and product. CO (g) + H₂O (g) Kp = 0.0611 at 2000K.
Consider the equilibrium system below. For this reaction, Kp = 205. If the equilibrium partial pressure of Cl2 is 0.050 atm and the partial pressure of NOCl is 0.095 M what is the equilibrium partial pressure of NO? 2 NO (g) + Cl2 (g) <-> 2 NOCl (g)