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Colt1911 [192]
3 years ago
15

The combustion of 1.00 mol of glucose, C6H12O6, releases 2820 kJ of heat. If 2.0 g of glucose is burned in a calorimeter contain

ing 1.0 kg of water, and the temperature increases by 3.5 oC, what is the heat capacity of the calorimeter?
Chemistry
1 answer:
DochEvi [55]3 years ago
3 0

Answer:

The heat capacity of the calorimeter is 4.76 kJ/°C

Explanation:

Step 1: Data given

1.00 mol of glucose releases 2820 kJ of heat

Mass of glucose = 2.0 grams

Mass of water = 1000 grams

The temperature increases with 3.5 °C

Step 2: Calculate moles

moles glucose = mass glucose / molar mass glucose

moles glucose = 2.0 grams / 180.16 g/mol

moles glucose = 0.0111 moles

Step 3: Calculate heat produced by the combustion

Heat produced = 2820 kJ/mol * 0.0111 moles

Heat produced = 31.302 kJ = 31302 J

Step 4: Calculate heat absorbed by the water

Q = m*c*ΔT

⇒ with m = the mass of water = 1000 grams

⇒ with c = the specific heat of water = 4.184 J/g°C

⇒ with ΔT = The change in temperature = 3.5 °C

Q = 1000 * 4.184 *3.5

Q = 14644 J absorbed by the water

Step 5: Calculate heat basorbed by the calorimeter

Q = 31302 - 14644 = 16658 J absorbed by the calorimeter

Step 6: Calculate the heat capacity of the calorimeter

c= 16658 J / 3.5 °C

c = 4759 J/°C = 4.76 kJ/°C

The heat capacity of the calorimeter is 4.76 kJ/°C

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fog

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3 years ago
A helium filled ballon had a volume of 8.50 L on the ground at 20.0 C and a pressure of 750.0 Torr. After the ballon was release
Marrrta [24]

Answer:

V_2=12.1L

Explanation:

Hello!

In this case, according to the given data of volume, pressure and temperature, it is possible to infer this problem can be solved via the combined gas law:

\frac{P_1V_1}{T_1} =\frac{P_2V_2}{T_2}

Thus, regarding the question, we evidence we need V2, but first we make sure the temperatures are in Kelvins:

T_1=20+273=293K\\\\T_2=-40+273=233K

Then, we obtain:

V_2=\frac{P_1V_1T_2}{T_1P_2}\\\\V_2=\frac{0.987atm*8.50L*233K}{293K*0.550atm}\\\\V_2=12.1L

Best regards!

5 0
2 years ago
If i have 4 moles of a gas at a pressure of 5 atm and a volume of 12 liters what is the temperature?
My name is Ann [436]

Answer:

182.70K

Explanation:

Using the general gas equation as follows:

PV = nRT

Where;

P = pressure (atm)

V = volume (L)

n = number of moles (mol)

R = 0.0821 Latm/Kmol

T = temperature (K)

Based on the provided information, P = 5 atm, V = 12L, n = 4 moles, T =?

PV = nRT

5 × 12 = 4 × 0.0821 × T

60 = 0.3284T

T = 60/0.3284

T = 182.70K

4 0
3 years ago
For the reaction H2O(g) + Cl2O(g) → 2HCIO(9), you know S rxn and Sosys and S° of HCIO(g) and of H2O(g). Write an expression that
Liono4ka [1.6K]

The expression that can be used to determine Cl2O(g) is ;

S_{cl_{2}o(g) } ^{o} = 2S_{HCIO(g)} ^{o} - S_{H_{2}O(g) }^{o} - \beta S_{rxn} ^{o}

<h3>Determine an expression that can be used to determine Cl2O(g)</h3>

The general expression for ΔS°rxn of a chemical reaction

ΔS°rxn = ∑mS°products - ∑nS°reactants

where ; m and n = stoichiometry coefficients

Considering the given reaction : H₂O(g) + Cl₂O(g) → 2HCIO (g)  

\betaS°rxn  = 2S_{HCIO(g)} ^{o} - S_{H_{2}O(g) } ^{o} - S_{Cl_{2}O } ^{o} ------- ( 2 )

Rearranging the equation above

S_{cl_{2}o(g) } ^{o} = 2S_{HCIO(g)} ^{o} - S_{H_{2}O(g) }^{o} - \beta S_{rxn} ^{o}

Hence we can conclude that The expression that can be used to determine Cl2O(g) is ;

S_{cl_{2}o(g) } ^{o} = 2S_{HCIO(g)} ^{o} - S_{H_{2}O(g) }^{o} - \beta S_{rxn} ^{o}

Learn more about stoichiometry : brainly.com/question/16060223

3 0
2 years ago
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