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miv72 [106K]
3 years ago
8

What is 1 Oz equal to in grams?

Chemistry
2 answers:
lakkis [162]3 years ago
4 0
1 Oz is 28.3495 grams

hope this helps!
pentagon [3]3 years ago
3 0

Conversion factor for ounces and grams.

<em>1 ounce is equal to approximately 28.4 grams. </em>

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At what temperatures is a reaction that has a positive change in entropy
Setler [38]

Answer:

the answer is A

I made a chart for AP chem if you want to refer to it.

3 0
3 years ago
Which of the following statements is true for an exothermic reaction?
shutvik [7]
The enthalpy change for an exothermic reaction is negative because heat is being released, so that takes out two of the responses. Since energy is being released into the surroundings due to the exothermic reaction, the potential energy of the products is lower than that of the reactants. Energy is being put in to make the reaction occur, but then that energy is all being released into the surroundings thus a lower potential energy level for the products
6 0
3 years ago
Read 2 more answers
Suppose 40.8g of copper(II) acetate is dissolved in 200.mL of a 0.70 M aqueous solution of sodium chromate.
Contact [7]

Answer:

0.42 M

Explanation:

The reaction that takes place is:

  • Cu(CH₃COO)₂ + Na₂CrO₄ → Cu(CrO₄) + 2Na(CH₃COO)

First we <u>calculate the moles of Na₂CrO₄</u>, using the <em>given volume and concentration</em>:

(200 mL = 0.200L)

  • 0.70 M * 0.200 L = 0.14 moles Na₂CrO₄

Now we <u>calculate the moles of Cu(CH₃COO)₂</u>, using its <em>molar mass</em>:

  • 40.8 g ÷ 181.63 g/mol = 0.224 mol Cu(CH₃COO)₂

Because the molar ratio of Cu(CH₃COO)₂ and Na₂CrO₄ is 1:1, we can directly <u>substract the reacting moles of Na₂CrO₄ from the added moles of Cu(CH₃COO)₂</u>:

  • 0.224 mol - 0.14 mol = 0.085 mol

Finally we <u>calculate the resulting molarity</u> of Cu⁺², from the <em>excess </em>cations remaining:

  • 0.085 mol / 0.200 L = 0.42 M

4 0
3 years ago
The pressure exerted by 1.5 mol of gas in a 13 L flask at 22 °C is ____ kPa
sukhopar [10]

Answer:

282.7KPa

Explanation:

Step 1:

Data obtained from the question.

Number of mole of (n) = 1.5 mole

Volume (V) = 13L

Temperature (T) = 22°C = 22 + 273°C = 295K

Pressure (P) =..?

Gas constant (R) = 0.082atm.L/Kmol

Step 2:

Determination of the pressure exerted by the gas.

This can be obtained by using the ideal gas equation as follow:

PV = nRT

P = nRT /V

P = 1.5 x 0.082 x 295 / 13

P = 2.79atm.

Step 3:

Conversion of 2.79atm to KPa.

This is illustrated below:

1 atm = 101.325KPa

Therefore, 2.79atm = 2.79 x 101.325 = 282.7KPa

Therefore, the pressure exerted by the gas in KPa is 282.7KPa

8 0
3 years ago
If 100 mL of a 12 M solution of HCl is diluted to a final volume of 500 mL, what would be the final concentration of the diluted
AURORKA [14]
Dilution formula:
mv = MV

where one side is concentration × volume BEFORE dilution and the other side is concentration × volume AFTER dilution. 

(100mL) × (12 M) = (500mL) × (X)
(1200 M·mL) = (500mL) × (X)
(1200 M·mL) / (500mL) = X
2.4 M = X

3 0
3 years ago
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