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2 years ago

The volume of a sample of gas, initially at 25 °C and 158 mL, increases to

Chemistry

1 answer:

Artist 52 [7]2 years ago

5 0

Answer:

The final temperature = 848.7 K or 575.7 °C

Explanation:

Step 1: Data given

Temperature = 25.0 °C = 298 K

Volume = 158 mL = 0.158 L

The volume increases to 450 mL = 0.450 L

The pressure is constant

Step 2: Calculate the final temperature

V1/T1 = V2/T2

⇒with V1 = the initial volume = 0.158 L

⇒with T1 = the initial temperature = 298 K

⇒with V2 = the increased volume = 0.450 L

⇒with T2 = the new temperature = TO BE DETERMINED

0.158 L / 298 K = 0.450 L / T2

T2 = 0.450 L / (0.158L/298K)

T2 = 848.7 T

The final temperature = 848.7 K or 575.7 °C

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Which one of these terms represents the chemistry definition and why are the other three wrong? Please help

motikmotik

Answer:

D. Fire

Explanation:

Fire represents that if any acid or chemical reaction occurs, there may be chances of fire/explosion occurring. Wind, sunlight and dust doesn't matter when it comes to experimenting with chemicals.

Hope it helped! Mark BRAINLIEST!

8 0

2 years ago

If 298 mL of 0.575 M CuCl2 is diluted into 750 mL, what is the concentration of new solution?

Sonja [21]

Answer:

<h3>The answer is 0.228 M</h3>

Explanation:

To find the concentration of new solution we use the formula

$C_1V_1 = C_2V_2$

where

C1 is the concentration of the stock solution

V1 is the volume is the volume of the stock solution

C_2 is the concentration of the diluted solution

V2 is the volume of the diluted solution

Since we are finding the the concentration of new solution

$C_2 = \frac{C_1V_1}{V_2} \\$

From the question

C1 = 0.575 M

V1 = 298 mL

V2 = 750 mL

We have

$C_2 = \frac{0.575 \times 298}{750} \\ = 0.228466666...$

We have the final answer as

Hope this helps you

4 0

3 years ago

Formic acid (HCO2H) has a dissociation constant of 1.8 x 10^-4 M. The acid dissociates 1:1. What is the [H+] if 0.35 mole of for

Tju [1.3M]

Initial [ HCO2H] = moles * volume
=0.35 moles * 1 L = 0.35 M

by using ICE table:

HCO2H ↔ H+ + HCO2-
initial 0.35 M 0 0
change - X +X +X
Equ (0.35 - X) X X

∴ Ka = [H+][HCO2-] / [HCO2H]

by substitution:

1.8 x 10^-4 = X^2 / (0.35-X) by solving for X

∴ X = 0.0079 or 7.9 x 10^-3

∴ [H+] = X = 7.9 x 10^-3 M

7 0

2 years ago

Carbon, hydrogen and ethane each burn exothermically in an excess of air. AHⓇ =-393.7 kJ mol. C(s) + O2(g) → CO2(g) H2(g) + % O2

Salsk061 [2.6K]

<u>Answer:</u> The $\Delta H^o_{rxn}$ for the reaction is 51.8 kJ.

<u>Explanation:</u>

Hess’s law of constant heat summation states that the amount of heat absorbed or evolved in a given chemical equation remains the same whether the process occurs in one step or several steps.

According to this law, the chemical equation is treated as ordinary algebraic expressions and can be added or subtracted to yield the required equation. This means that the enthalpy change of the overall reaction is equal to the sum of the enthalpy changes of the intermediate reactions.

The chemical equation for the reaction of carbon and water follows:

$2C(s)+2H_2(g)\rightarrow C_2H_4(g)$ $\Delta H^o_{rxn}=?$