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anygoal [31]
3 years ago
15

When a 8 gram slice of bread is burned under a beaker of 4500 grams of water, it heats up the water by 1.3 degrees Celsius. The

specific heat of water is 1 cal/g degree C. How many calories does this slice of bread contain
Chemistry
1 answer:
dezoksy [38]3 years ago
5 0

Answer:

5850\ \text{cal}

Explanation:

m = Mass of water = 4500 g

c = Specific heat of water = 1\ \text{cal/g}^{\circ}\text{C}

\Delta T = Change in temperature of water = 1.3^{\circ}\text{C}

Heat is given by

q=mc\Delta T\\\Rightarrow q=4500\times 1\times 1.3\\\Rightarrow q=5850\ \text{cal}

A slice of the bread contains 5850\ \text{cal}.

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find the moles of O2 used = mass/molar mass

= 40 g/32g/mol = 1.25  moles

write the reacting equation
4Na+ O2 = 2Na2O

by use of mole ratio between Na to O2 which is 4 :1

the moles of Na = 1.25 x 4 = 5 moles

mass of Na = mass x molar mass

=  5 moles x 23 g /mol= 115  moles
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Determine the molecular formula for the compound with a molar mass of 46.08 g/mol and the following percent compostion:
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Answer:

      \large\boxed{\large\boxed{CH_6N_2}}

Explanation:

<u><em>1. First determine the empirical formula.</em></u>

a) Base: 100 g of compound

             mass       atomic mass      number of moles

                g                g/mol                    mol

C           26.06            12.011             26.06/12.011   = 2.17

H           13.13              1.008              13.13/1.008    =  13.03

N           60.81             14.007            60.81/14.007 = 4.34

b) Divide every number of moles by the smallest number: 2.17

mass       number of moles        proportion

C                  2.17/2.17                         1

H               13.03/2.17                         6

N                4.34/2.17                          2

c) Empirical formula

      CH_6N_2

d) Mass of the empirical formula

      1\times 12.011g/mol6+6\times 1.008g/mol+2\times 14.007g/mol=46.07g/mol

<u><em>2. Molecular formula</em></u>

Since the mass of one unit of the empirical formula is equal to the molar mass of the compound, the molecular formula is the same as the empirical formula:

                   CH_6N_2

6 0
3 years ago
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