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BabaBlast [244]
3 years ago
12

A compound has the empirical formula CH2O and a gram-formula mass of 60. grams per mole. What is the molecular formula of this c

ompound?
(1) CH2O (3) C3H8O
(2) C2H4O2 (4) C4H8O4
Chemistry
1 answer:
AlladinOne [14]3 years ago
4 0
We already know the molar mass of C is 12.01g/mol, of H is 1.008 g/mol, and of O is 16g/mol.

If the molecular formula were also the empirical formula (which is CH2O), then it would have a molar mass of:
12.01g/mol +2*(1.008g/mol)+ 16g/mol= 30.03g/mol

However, the actual molar mass of the molecular formula is 60.g/mol, which is about twice as large as 30.03g/mol. Therefore, we have to multiply the empirical formula by 2.

The molecular formula of this compound is (2) C2H4O2.

Hope this would help~

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5 0
3 years ago
Use the following balanced reaction to solve 1-3:
tino4ka555 [31]

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2 years ago
A solution is prepared at that is initially in chloroacetic acid , a weak acid with , and in potassium chloroacetate . Calculate
ratelena [41]

Answer:

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Explanation:

There is some info missing. I think this is the original question.

<em>A solution is prepared at 25 °C that is initially 0.38 M in chloroacetic acid (HCH₂ClCO₂), a weak acid with Ka= 1.3 x 10⁻³, and 0.44 M in sodium chloroacetate (NaCH₂CICO₂). Calculate the pH of the solution. Round your answer to 2 decimal places.</em>

<em />

We have a buffer system formed by a weak acid (HCH₂ClCO₂) and its conjugate base (CH₂CICO₂⁻ coming from NaCH₂CICO₂). We can calculate the pH using the Henderson-Hasselbalch equation.

pH = pKa + log [CH₂CICO₂⁻]/[HCH₂ClCO₂]

pH = -log 1.3 x 10⁻³ + log (0.44 M/0.38 M)

pH = 2.94

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Marta_Voda [28]
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3 0
2 years ago
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Answer:

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