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torisob [31]
4 years ago
11

In a reaction that produces carbon dioxide, the theoretical yield is 59 grams. During the experiment, the reaction actually prod

uced 52.9 grams of carbon dioxide. Determine the percent yield.
Chemistry
1 answer:
Roman55 [17]4 years ago
4 0

Answer:

mole ratio, which is equivalent to a 1;1 mole ratio, to a gram ratio. This means that when the reaction consumes 84.03 g of carbon monoxide, it should theoretically produce 132.03 g of carbon dioxide. Use this gram ratio to calculate the theoretical yield for your reaction.

Explanation:

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4 0
3 years ago
Complete the lewis structures of the atoms and ions by adding electrons, as needed.
Lana71 [14]
Hope this helps! Na+ lost an electron, so I just left a "+" symbol to show that, and fluorine gained an electron, hence the "-" symbol.

3 0
4 years ago
Read 2 more answers
What is an example of a Low Energy-created depositional environment?
sweet-ann [11.9K]

Answer:

River flood plains, swamps, lakes, lagoons, marshes, and offshore.

Explanation:

Slow-moving currents prevent coarse-grained sediment from migrating into low-energy depositional environments. Fine materials can be carried long distances before they can settle out in the absence of waves and currents.

4 0
3 years ago
A 260.0 −mL buffer solution initially contains 2.5×10−2 M of HCHO2 and 2.5×10−2 M of NaCHO2
FinnZ [79.3K]

The mass of HCHO2 and NaCHO2 to be added to the buffer solution are 0.23g and 0.44g respectively

Data;

  • Volume of solution = 260mL
  • conc. of HCHO2 = 2.5*10^-2M
  • conc. of NaCHO2 = 2.5*10^-2M

<h3>Mass of Reagent Added</h3>

To calculate the mass of reagent added,  let's start with HCHO2

The mass of HCHO2 to be added is the number of moles of HCHO2 multiplied by it's molar mass.

260*10^-^3 * 2.5*10^-^2 * 46 = 0.229 = 0.23g

The mass of NaCHO2 to be added in the buffer solution is

260*10^-^3*2.5*10^-^2*68 = 0.442 = 0.44g

The mass of HCHO2 and NaCHO2 to be added to the buffer solution are 0.23g and 0.44g respectively

Learn more about buffer solution here;

brainly.com/question/22390063

3 0
2 years ago
1.00 L of a gas at STP is compressed to 473mL. What is the new pressure of gas?
Ratling [72]

Hello!

1.00 L of a gas at STP is compressed to 473 mL. What is the new pressure of gas?

  • <u><em>We have the following data:</em></u>

Vo (initial volume) = 1.00 L  

V (final volume) = 473 mL → 0.473 L  

Po (initial pressure) = 1 atm (pressure exerted by the atmosphere - in STP)  

P (final pressure) = ? (in atm)

  • <u><em>We have an isothermal transformation, that is, its temperature remains constant, if the volume of the gas in the container decreases, so its pressure increases. Applying the data to the equation Boyle-Mariotte, we have:</em></u>

P_0*V_0 = P*V

1*1 = P*0.473

1 = 0.473\:P

0.473\:P = 1

P = \dfrac{1}{0.473}

\boxed{\boxed{P \approx 2.11\:atm}}\:\:\:\:\:\:\bf\green{\checkmark}

<u><em>Answer:  </em></u>

<u><em>The new pressure of the gas is 2.11 atm  </em></u>

___________________________________

\bf\blue{I\:Hope\:this\:helps,\:greetings ...\:Dexteright02!}\:\:\ddot{\smile}

3 0
3 years ago
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