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NISA [10]
3 years ago
8

A sample of tin (Cp = 0.227 J/g•°C) is placed in a freezer. Its temperature decreases from 15.0°C to −10.0°C as it releases 543

J of energy. What is the mass of the sample? Round your answer to three significant figures.

Chemistry
2 answers:
Andreas93 [3]3 years ago
8 0
We know, Q = m.c.Δt
m = Q / c.Δt

Here, Q = 543 J
c = 0.227 J/g C
Δt = 15-(-10) = 25 C

Substitute their values,
m = 543 / 0.227 * 25
m = 543 / 5.675
m = 95.68 g

In short, Your Answer would be 95.68 gram

Hope this helps!
pshichka [43]3 years ago
8 0

Answer:

see attached picture

Explanation:

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Answer:

Final molarity of ammonium cation in the solution = 0.16 M

Explanation:

Complete Question

Suppose 2.59 g of ammonium nitrate is dissolved in 200. mL of a 0.40M aqueous solution of sodium chromate. Calculate the final molarity of ammonium cation in the solution. You can assume the volume of the solution doesn't change when the ammonium nitrate is dissolved in it. Be sure your answer has the correct number of significant digits.

Solution

2NH₄NO₃ + Na₂CrO₄ → (NH₄)₂CrO₄ + 2NaNO₃

We first convert the given parameters to number of moles

Number of moles = (Mass/Molar mass)

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Number of moles = (Concentration in mol/L) × (Volume in L)

Number of moles of Na₂CrO₄ = 0.4 × 0.2 = 0.08 Mole

2 moles of NH₄NO₃ react with 1 mole of Na₂CrO₄

So, it it evident that NH₄NO₃ is the limiting reagent as it is in short supply in the amount needed for the reaction.

So, the number of moles of ammonium ion in the product is also 0.03224 mole.

Molarity = (Number of moles)/(Volume L)

Molarity of ammonium ion = (0.03224/0.2) = 0.1612 mol/L = 0.16 M

Hope this Helps!!!

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