1.A hydrocarbon 0.106g when burnt in air gave 0.364g of CO2 and .596g of water.

Question

1.A hydrocarbon 0.106g when burnt in air gave 0.364g of CO2 and .596g of water. The molar mass of the compound is 256.4g/mol. What is the empirical and molecular formula of the compound? The atomic mass in g/mol C=12 H= 1.0 O= 16.0

2.What is the molarity of a solution prepared by dissolving 22.5 X10^-3 g of K2 CO3 in 750mls of water. Wht is the concentraition of eah ions in the solutions? Atomic mass of K=39 C=12 O=1

3.What volume of 0.007M solution of Li2CO3, in mililiters contains 14.776g of K2CO3 atomic mass K=39 C=12 O=16

4.3.694g of a mixture of ZnSO4 and ZnSO4 6H20 on heating leaves behind a residue of ZnSO4 weighing 2.614g accorind to the reaction ___ZnSO4 * 6H2O yield _ZnS04+ ___H2O

What is the mass percent of ZnSO4*6H2O in the original sample? Atomic Mass is g/mol Zn=65.4 H=1 O=16 S=32

5. 220.0g g of CaO is reacted with 330g of NH4Cl to yield 121.5g of NH3 according o reaction

_NH4Cl+___CaO yield _NH3+___CaCl2+ _H20

atomic mass in g/mol N=14 Cl=35 O=16 H=1 Ca=40

a.The limiting reagent

b.theoretical yield

c.percent yield

d. the amount of unused excess reagents left behind

6.Calculate the percent abundance and the average chemical atomic mass of Sr given the follwing information Mg-24 mass 23.985042 amu and 78.99 percent abundance, Mg-25 mass 24.985837 amu, Mg-26 mass 25.982593 amu and 11.01 percent abundance

Explanation / Answer

molarity = 22.5x10^-3 x 1000/138.20 x 750

molarity = 22.5/103650

molarity = 2.1707x10^-4

molarity = 0.021707x10^-2M

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