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3 years ago

3. A 4.00 gram sample of solid gold was heated from 274K to 314K. How much energy was involved?

1 answer:

3 0

Q = mcΔT = (4.00 g)(0.129 J/g•°C)(40.85 °C - 0.85 °C)
Q = 20.6 J of energy was involved (more specifically, 20.6 J of heat energy was absorbed from the surroundings by the sample of solid gold).

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kogti [31]

In the given reaction, the substance that is the base of the reaction is $CaSO_4$ . The correct option is C.

The base is a slippery liquid that is bitter and turns red litmus paper to blue.

Bases react with acids to form salts.

Then bases have pH above 7.

Examples of bases are calcium carbonate, sodium hydroxide, etc.

Thus, the correct option is C.

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3 years ago

Which of the following is characteristic of non-metals?

IgorC [24]

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A student titrated a 25.00-mL sample of a solution containing an unknown weak, diprotic acid (H2A) with N2OH. If the titration r

lakkis [162]

<u>Answer:</u> The concentration of weak acid is $3.674\times 10^{-2}M$

<u>Explanation:</u>

To calculate the concentration of acid, we use the equation given by neutralization reaction:

$n_1M_1V_1=n_2M_2V_2$

where,

$n_1,M_1\text{ and }V_1$ are the n-factor, molarity and volume of acid which is $H_2A$

$n_2,M_2\text{ and }V_2$ are the n-factor, molarity and volume of base which is NaOH.

We are given:

$n_1=2\\M_1=?M\\V_1=25.00mL\\n_2=1\\M_2=0.1036M\\V_2=17.73mL$

Putting values in above equation, we get:

$2\times M_1\times 25.00=1\times 0.1036\times 17.73\\\\M_1=\frac{1\times 0.1036\times 17.73}{2\times 25.00}=3.674\times 10^{-2}M$

Hence, the concentration of weak acid is $3.674\times 10^{-2}M$

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3 years ago

Given the following unbalanced thermochemical equation, how much heat will be released from the combustion of 45.5 grams of CH4

AnnyKZ [126]

CH4 + 2O2 → CO2 + 2H2O + 890 kJ

MM of CH4 = (12.01 + 4x1.008) g/mol = 16.04 g/mol

Moles of CH4 = 45.5 g CH4 x (1 mol CH4/16.04 g CH4) = 2.837 mol CH4

q = 2.837 mol CH4 x (890 kJ/1 mol CH4) = 2520 kJ

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4 years ago