Calcium carbonate decomposes at high temperatures to give calcium oxide and carbon dioxide as shown below. CaCO3(s) CaO(s) + CO2(g) The Kp for this reaction is 1.16 at 800°C. A 5.00 L vessel containing 10.0 g of CaCO3(s) was evacuated to remove the air, sealed, and then heated to 800°C. Ignoring the volume occupied by the solid, what will be the mass of the solid in the vessel once equilibrium is reached? Multiple Choice O 6.9 g of solid 7.1 g of solid 7.3 g of solid 7.5 g of solid None of the above

Calcium carbonate decomposes at high temperatures to give calcium oxide and carbon dioxide as shown below. CaCO3(s) CaO(s) + CO2(g) The Kp for this reaction is 1.16 at 800°C. A 5.00 L vessel containing 10.0 g of CaCO3(s) was evacuated to remove the air, sealed, and then heated to 800°C. Ignoring the volume occupied by the solid, what will be the mass of the solid in the vessel once equilibrium is reached? Multiple Choice O 6.9 g of solid 7.1 g of solid 7.3 g of solid 7.5 g of solid None of the above

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

Reaction of carbon disulfide with hydrogen gas at 960 °C is a reversible reaction presented as follows CS2 (g) + 4H2 (g) ----> CH4 (g) + 2H2S (g)a. If the reaction was done in a 1.00-L evacuated vessel with 1.250 moles of CS₂ and 4.000 moles of H₂ initially, calculate the equilibrium constant if the amount of H₂S as it reached equilibrium was 1.670 moles.b. If the volume of the vessel was decreased to 0.500L, how much H₂S would be produced?
part d and e
consider the following exothermic reaction at 0.00 °C and 1.00 atm SeO4 (g) ⇌ Se(g) + O2(g) , kc = 2.4 ×10-6 The reaction contains [SeO4] = 0.100 M, [Se] = 0.0034 M, [O2] = 0.0022 MWhat is the value of KP for this reaction?
Consider the following reaction:2HI(g) ⇄ H2(g) + I2(g)At 500 K, the equilibrium constant, Kp is 0.049. A 1.50 L container at 500 K is initially filled with 0.809 mol of HI and allowed to equilibrate. What is the equilibrium concentration of H2(g)?
Phosphine gas (PH3), decomposes by the reaction shown below. A total pressure of 0.64 atm of pure phosphine gas was placed in a sealed 1.00-L flask at 298 K. After equilibrium was attained, the total pressure inside the flask was found to be 0.93 atm. Calculate the mass of solid phosphorous in the flask. PH3(g) <--> P(s) + 3 H2(g)
Consider the reaction: 2HI(g) ⇀ H2(g)+I2(g). At 500 C∘, a flask initially has all three gases, each at a partial pressure of 0.200 atm. When equilibrium is established, the partial pressure of HI(g) is determined to be 0.480 atm. a. Calculate the Kp for the reaction b. What is the equilibrium partial pressure of H2(g) and I2(g)? c. What is ΔG⊖reaction?
Matak
tab esc An evacuated reaction vessel is filled with 0.80 atm of N and 1.68 atm 2 of Br. When equilibrium is established according to the reaction below, there are 1.42 atm of Br, remaining in the vessel. What is Kp for this reaction? 2 2 NBr. (g) = N₂(g) + 3 Br₂ (g) ! Q 2 F2 W #3 3 20 F3 E $ 4 888 R 67 80 % 5 Question 17 of 21 F5 < MacBook Air 6 F6 Y & 7 F7 U 8 F8 ( 9 F9 1 4 7 +/- O O 2 LO 5 4 F10 11.6 P 3 8 9 CO 6 0 F11
11. PLease refer to the attached photo. THank youuu
The equilibrium constant (Kp) is 0.11 at a particular temperature for the reaction: N204(9) = 2NO2(9) Given the following sets of initial conditions, what is the net change that must occur for the reaction to reach equilibrium? Does the reaction shift left to reach equilibrium, does the reaction shift right to reach equilibrium or is the reaction at equilibrium at these initial concentrations so no net change will occur? A. PNO, = 0.105 atm, PN,0, = 0.146 atm В. PNO, = 0.093 atm, PN,0, = 0.054 atm С. PNO, = 0.180 atm, PN,0, = 0.134 atm %3D D. PNO, = 0.088 atm, PN,0, = 0.07 atm Е. PNO, = 0.055 atm, PN,0, = 0.06 atm %3D %D A. right B. left C. left D. equilibrium left right E. > >
At a particular temperature, Kp = 0.390 for the reaction N₂04(9) 2NO₂(g) A flask containing only NO2(g) at an initial pressure of 6.00 atm is allowed to reach equilibrium. Calculate the total pressure in this flask at equilibrium. 3.494 atm You are correct. Your receipt no. is 153-8518 Ⓒ With no change in the amount of material in the flask, the volume of the container in question is increased to 4.000 times the original. Assuming constant temperature, calculate the (new) total pressure, at equilibrium. 8.7e-1 atm Previous Tries Submit Answer Incorrect. Tries 7/99 Previous Tries
At 150°C, Kp = 1.2x10- for the reaction 12(g) + Br2(g) 5 2Brl(g). A rigid cylinder at that temperature contains 0.127 atm of bromine, 0.134 atm of iodine, and 1.055 atm of bromine monoiodide. What is the value of the reaction quotient, Qp? O 55.2 62.0 O 65.4 O 88.3