00 96 96 %24 # m Be sure to answer all parts. How many liters does each of the following quantities of O, occupy at STP: (a) 6.1 mol; (b) 0.79 mol;? x 10 (b) L. IIO 2 4.

Assume all reations involving gases proceed at STP.  1) 2Li + 2 H2) 2 LiOH +H2... If 4.4247 moles of Li are reacted, how many moles of LiOH will be reducd?

Carry only 1 decimal point on all atomic weights (X.X). What is the mole fraction of O2 in a mixture that is 283.6 g N2, 145.1 g O2, and 5.111 g CO2?

2 H3PO4(s) --> 3 H2(g) + 2 P(s) + 4 O2(g) Using the reaction above, show step by step how many liters of oxygen can be created if I start with 0.7156 grams of H3PO4 solid at STP?

Please don't provide handwriting solution

[6] Magnesium carbonate reacts with hydrochloric acid to form the products shown below. If 45.0 g of MgCO; reacted with 50 ml of 0.1000M HCl what volume of CO2 would be produced at STP. MgCO3(s) + 2HCI (aq) → MgCl2(aq) + H2O(1) + CO2(g)

6. If 15.00g of Mg¿(SO4)3 is reacted with 32.25mL of o.2038M of AGNO3 to produce Mg(NO3)2 and Ag.SO4, answer the following questions.

A sample containing a mixture of SrCl, · 6 H,0 (MW = 266.62 g/mol) and CSCI (MW = 168.36 g/mol) originally weighs 1.6017 g. Upon heating the sample to 320 °C, the waters of hydration are driven off SrCl, · 6 H,0, leaving the anhydrous SrCl,. After cooling the sample in a desiccator, it has a mass of 1.1433 g. Calculate the weight percent of Sr, Cs, and Cl in the original sample. 320 °C SrCl, · 6 H,0(s)- SrCl, (s) + 6 H,O(g) wt% Sr = wt% Cs = wt% CI =

(ans: -7.50 x 10 ) one mole of sucrose). Imol %3D 9reaction=n AH %3D %3D (ans: -5.64 x 10 kJ/mol) Calcium chloride and sodium hydroxide react according to the equation: CaCl(aq) + 2 NaOH(aq) → Ca(OH),(s) +2 NaCl(aq) What volume of 2.00 M NaOH would be needed to react with 50.0 mL of 1.50 M CaCl,? a, 017 (ans: 75.0 mL) b) When 50.0 mL of 1.50 M CaCl, solution and 80.0 mL of 2.00 M NAOH solution (i.e., 5.0 mL more than calculated in part (a)) both initially at 22.3°C are mixed in a coffee-cup calorimeter with a calorimeter constant of 12.8 J/ C, the temperature fell to 20.0°C. If the density of the reaction mixture is 1.03 g/mL and its specific heat 3.94 J/g°C, calculate the heat absorbed hv the reaction. (ans: 1.24 x 103) c) Calculate AH (in kJ per mole of Ca(OH)2 formed) for the reaction. (ans: 1.6 x 10' kJ/mol)

Please see question 28, just the top one. I figure in this system the pressure is changing and my answer is the original pressure divided by the final pressure is equal to X.  Do I have this correct?     pv= nRT      N and T and R are constants   thus P1V1 = P2V2.