< Question 5 of 9 > At a certain temperature and pressure, 1 L of Co,...
< Question 7 of 9 > A sample of an ideal gas has a volume of 2.23 L at 2.80 x 102 K and 1.13 atm. Calculate the pressure when the volume is 1.30 L and the temperature is 304 K. P = atm
Question 10 of 11 > At a certain temperature, 0.880 mol SO, is placed in a 4.50 L container. 2 503(g) = 2 802(g) + O2(g) At equilibrium, 0.100 mol O, is present. Calculate Ko.
At a certain temperature and pressure, 1 L of Co, gas weighs 1.36 8. What is the mass of 1 L of N, gas at the same temperature and pressure? mass of 1 L of N, 1.16
< Question 19 of 22 > Calculate the density of carbon monoxide, CO, at STP. Assume ideal behavior. density: g/L Question 20 of 22 > What pressure is exerted by 804.4 g of CH4 in a 0.760 L steel container at 209.8 K? P= atm < Question 21 of 22 > The combustion of octane, CHg, proceeds according to the reaction shown. 2C7H18(1) + 25 02(g) → 16 CO2(g) + 18 H2O(1) If 603 mol of octane combusts, what volume...
assignment Score: 300/1100 Resources Hint Check Answer Question 11 of 11 > At a certain temperature and pressure, 1 L of Co, gas weighs 1.45 g. What is the mass of 1 L of CH, gas at the same temperature and pressure? mass of 1 L of CH :
Question 10 of 22 A 4.05 g sample of an unknown gas at 35 °C and 1.05 atm is stored in a 2.15 L flask. What is the density of the gas? density: 1.88372 g/L What is the molar mass of the gas? molar mass: g/mol Incorrect Question 14 of 22 A gas mixture is made by combining 6.7 g each of Ar, Ne, and an unknown diatomic gas. At STP, the mixture occupies a volume of 15.14 L. What...
(5) Use induction to show that Ig(n) <n for all n > 1.
< Question 11 of 22 At a certain temperature, a 25.0-L container holds four gases in equilibrium. Their masses are 3.5 g SO 4.6 , 25.03 N,, and 0.98 g NO. What is the value of the equilibrium constant at this temperature for the reaction of SO, with N20 to form SO, and N7 Make sure you balance the reaction using the lowest whole number coefficients K =
Collecting Gas over water Sodium metal reacts with water to produce hydrogen gas according to the following equation: 2Na(s) + 2H20(1)—>2NaOH(aq) + H2(g) The product gas, H2, is collected over water at a temperature of 25 °C and a pressure of 746 mm Hg. If the wet H2 gas formed occupies a volume of 7.28 L, the number of grams of H, formed is g. The vapor pressure of water is 23.8 mm Hg at 25 °C.
< Question 11 of 11 > Calculate the value of K, for the equation C(s) + CO,(g) = 2 CO(g) Kp = ? given that at a certain temperature C(s) + 2H2O(g)=CO,(g) + 2 H (g) Kp1 = 3.41 HL8) + CO,(8)=H,Og) + CO(g) Kp2 = 0.611