I have 6 questions that Im beyond confused on solving. Some one please help me a

Question

I have 6 questions that Im beyond confused on solving. Some one please help me and give me step by bzstep instructions please.

1. What mass of magnesium (II) chloride must react with sulfuric acid to release 49.5 mL of hydrogen gas at STP? Based on this equation.

MnCI2(s)+ H2SO4 (aq)= MnSO4 (aq)+ 2 HCI (g)

2. What volume of sulfur dioxide gas reacts with 25.0 mL of O2, with this equation is SO2 (g) + O2 (g)= SO3 (g). The reaction conditions are 875 degress celcius and 1.00 atm pressure.

3. If 1.00 mol of nitrogen monoxide gas and 2.00 mol of oxygen gas, what is the limiting reactant and how many moles of NO2 are produced according to the equation:  2 NO(g) + O2 (g)= 2 NO2(g)

4. If 1.00 mol of ethane gas and 3.00 mol of oxygen reacts, what is the limiting reactant and how many moles of water are produced according to the equation: 2 C2H6 (g)+ 7 02 (g)= 4 CO2 (g)+ 6 H20  (g)

5. If 37.5 g of molten iron (III) oxide reacts with 175 g of aluminum according to this equation: Fe203 (l)+ Al (l)= Fe (l) + Al203 (s). What is the mass of iron produced?

6. If 1.25 L of sulfur dioxide gas reacts with 3.00ml of oxygen according to this equation. SO2 (g)+ 02 (g)= SO3 (g). What is the volume of sulfur trioxide gas produced? Assume all gases are at the same temperature and pressure.

Explanation / Answer

1.2HCl gas gives H2 i.e 1 mole H2 is from 2 moles HCl therefore 49.5 ml = 49.5/22400 since 1 mole of H2 gas at STP occupies 22400 ml thus we get the moles of HCl reqd and from that we get the moles of MnCl2 required which gmultiplied by the molar mass of MnCl2 gives the ans 2. at the given reaction conditions we apply gas eqn PV = NRT to find no of moles of O2 being used and thus from the stoichiometry we get the moles of sulphur dioxide and its volume

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