Answer:
For number 5 it is the 2nd one some stants has a mass of 1.25 g And the 2nd 1 number 6It is the 1st 1A subject has a melting point of 40
Answer:
Explanation:
Unclear question.
I infer you want a clear rendering, which reads;
A 258.4 g sample of ethanol (C2H5OH) was burned in a calorimetric pump using a Dewar glass. As a consequence, the water temperature rose to 4.20 ° C.
If the heat capacity of the water and the surrounding glass was 10.4 kJ / ° C, calculate the heat of combustion of one mole of ethanol.
Answer:
3M
Explanation:
moles ÷ liters = molarity
4.8 ÷ 1.6 = 3M
Molar mass (NH₄)₂CO₃ = <span>96.09 g/mol
1 mole ---------> 96.09 g
0.500 moles ----> ?
0.500 * 96.09 = 48.045 g of </span><span>(NH₄)₂CO₃
hope this helps!
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