Question

Question 4 (1 point) A compound with a molecular mass of 283.88 g/mol is found to contain 43.64 %P and 56.36% O. What is the molecular formula of this compound? OPO4 OP203 P205 OP4010 OPAOG Question 5 (1 point) If (4.544x10^1) g of oxygen react with (4.81x10^1) g of carbon monoxide to form carbon dioxide. What mass of carbon dioxide forms? Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: Answer

Answer 1

4)

we have mass of each elements as:

P: 43.64 g

O: 56.36 g

Divide by molar mass to get number of moles of each:

P: 43.64/30.97 = 1.409

O: 56.36/16.0 = 3.522

Divide by smallest:

P: 1.409/1.409 = 1

O: 3.522/1.409 = 2.5

Multiply by 2 to get simplest whole number ratio:

P: 1*2 = 2

O: 2.5*2 = 5

So empirical formula is:P2O5

Molar mass of P2O5,

MM = 2*MM(P) + 5*MM(O)

= 2*30.97 + 5*16.0

= 141.94 g/mol

Now we have:

Molar mass = 283.88 g/mol

Empirical formula mass = 141.94 g/mol

Multiplying factor = molar mass / empirical formula mass

= 283.88/141.94

= 2

So molecular formula is:P4O10

Answer: P4O10

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