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RideAnS [48]
3 years ago
5

A hot pack contains 715g of water at 60 degrees Celsius. If the water cools to body temperature, how many kilocalories of heat c

ould be transferred to an inflamed ankle?
Chemistry
1 answer:
11Alexandr11 [23.1K]3 years ago
8 0

<u>Answer:</u>

<em>49822 joules of heat can be transferred to ankle from heat bag. </em>

<u>Explanation:</u>

We know that average body temperature should be <em>37 degree centigrade </em>

Hot water bag has 715 grams of water present in it. Specific heat of 1 gram of water is 4.18 joules per gram per degree centigrade. 715 grams will have 715 \times 4.18= 2988.7 j

The degree of water that is given is 60° hence specific heat becomes179322 \ j

<em>Specific heat of body at 37° centigrade will be = 129500 \ j</em>

<em>The amount of heat that can be transferred from hot bag will be 179322 - 129500 = 49822 \ j</em>

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4960000000 pm

Explanation:

4.96*1000000000= 4960000000

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What makes a substance pure?
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Burning 12.00 g of an oxoacid produces 17.95 g of carbon dioxide and 4.87 g of water. Consider that 0.25
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Answer: The molecular formula will be C_6H_6O_6

Explanation:

Mass of CO_2 = 17.95 g

Mass of H_2O= 4.87 g

Molar mass of carbon dioxide = 44 g/mol

Molar mass of water = 18 g/mol

For calculating the mass of carbon:

In 44g of carbon dioxide, 12 g of carbon is contained.

So, in 17.95 g of carbon dioxide, =\frac{12}{44}\times 17.95=4.89g of carbon will be contained.

For calculating the mass of hydrogen:

In 18g of water, 2 g of hydrogen is contained.

So, in 4.87 g of water, =\frac{2}{18}\times 4.87=0.541g of hydrogen will be contained.

Mass of oxygen in the compound = (12.00) - (4.89+0.541) = 6.57 g

Mass of C = 4.89 g

Mass of H =  0.541 g

Mass of O = 6.57 g

Step 1 : convert given masses into moles.

Moles of C =\frac{\text{ given mass of C}}{\text{ molar mass of C}}= \frac{4.89g}{12g/mole}=0.407moles

Moles of H=\frac{\text{ given mass of H}}{\text{ molar mass of H}}= \frac{0.541g}{1g/mole}=0.541moles

Moles of O=\frac{\text{ given mass of O}}{\text{ molar mass of O}}= \frac{6.57g}{16g/mole}=0.410moles

Step 2 : For the mole ratio, divide each value of moles by the smallest number of moles calculated.

For C =\frac{0.407}{0.407}=1

For H =\frac{0.541}{0.407}=1

For O = \frac{0.410}{0.407}=1

The ratio of C : H : O = 1: 1  : 1

Hence the empirical formula is CHO.

Hence the empirical formula is CHO

The empirical weight of CHO = 1(12)+1(1)+1(16)= 29 g.

If 0.25 moles has mass of 44.0 g

Thus 1 mole has mass of = \frac{44.0}{0.25}\times 1=176g

Thus molecular mass is 176 g

Now we have to calculate the molecular formula.

n=\frac{\text{Molecular weight }}{\text{Equivalent weight}}=\frac{176g}{29g}=6

The molecular formula will be=6\times CHO=C_6H_6O_6

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