Calculate the final temperature when 50.0 mL of water at 65.0 °C are added to 25 mL of water at 25.0 °C.

Chemistry

1 answer:

jok3333 [9.3K]2 years ago

7 0

Answer:

x=51.66

Explanation:

1 ml = 1 gram

(mass) (Δt) (Cp) = (mass) (Δt) (Cp)

Substituting values into the above, we then have:

(25)(25-x)(4.184)=(50)(x-65)(4.18)

Solve for x

x= 51.6667

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The decomposition reaction of N2O5 in carbon tetrachloride is 2N2O5−→−4NO2+O2. The rate law is first order in N2O5. At 64 °C the

Mademuasel [1]

Answer:

(a) rate = 4.82 x 10⁻³s⁻¹ [N2O5]

(b) rate = 1.16 x 10⁻⁴ M/s

(d) rate = 5.80 x 10⁻⁵ M/s

Explanation:

We are told the rate law is first order in N₂O₅, and its rate constant is 4.82 x 10⁻³s⁻¹ . This means the rate is proportional to the molar concentration of N₂O₅, so

(a) rate = k [N2O5] = 4.82 x 10⁻³s⁻¹ x [N2O5]

(b) rate = 4.82×10⁻³s⁻¹ x 0.0240 M = 1.16 x 10⁻⁴ M/s

(c) Since the reaction is first order if the concentration of N₂O₅ is double the rate will double too: 2 x 1.16 x 10⁻⁴ M/s = 2.32 x 10⁻⁴ M/s

(d) Again since the reaction is halved to 0.0120 M, the rate will be halved to

1.16 x 10⁻⁴ M/s / 2 = 5.80 x 10⁻⁵ M/s

3 0

3 years ago

Read 2 more answers

At the Henry's Law constant for carbon dioxide gas in water is . Calculate the mass in grams of gas that can be dissolved in of

Dvinal [7]

The question is incomplete, here is the complete question:

At 25°C Henry's Law constant for carbon dioxide gas in water is 0.031 M/atm . Calculate the mass in grams of gas that can be dissolved in 425. mL of water at 25°C and at a partial pressure of 2.92 atm. Round your answer to 2 significant digits.

<u>Answer:</u> The mass of carbon dioxide that can be dissolved is 1.7 grams

<u>Explanation:</u>

To calculate the molar solubility, we use the equation given by Henry's law, which is:

$C_{CO_2}=K_H\times p_{CO_2}$