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Paha777 [63]
2 years ago
5

I swear, everyone just ignores my question, but I'm going to ask anyways. A beaker is filled with 5.4 grams of Oxygen gas in a f

ixed volume of 4.0 liters. One of the valves opened and there remains only 1.7 grams of Oxygen gas, what is the new volume of gas?
Chemistry
1 answer:
Verizon [17]2 years ago
7 0

Answer:

2 P2 (1.2 atm =157 one. 8. A gas with a volume of 4.0 L

Explanation:

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Which is the empirical formula for a compound that contains 64.75g nitrogen and 185.25 oxygen
Svetach [21]

Answer:

What is the formula for a compound that contains 64.75 g nitrogen and 185.25 g oxygen? D. N2O5

The name of a hydrate is calcium chloride dihydrate. What is its formula? B. CaCl2 x 2H20

Explanation:

BRAINLIEST PLZZZZ

5 0
3 years ago
onsider the following reaction: CaCN2 + 3 H2O → CaCO3 + 2 NH3 105.0 g CaCN2 and 78.0 g H2O are reacted. Assuming 100% efficiency
mestny [16]

Answer : The excess reactant is, H_2O

The leftover amount of excess reagent is, 7.2 grams.

Solution : Given,

Mass of CaCN_2 = 105.0 g

Mass of H_2O = 78.0 g

Molar mass of CaCN_2 = 80.11 g/mole

Molar mass of H_2O = 18 g/mole

Molar mass of CaCO_3 = 100.09 g/mole

First we have to calculate the moles of CaCN_2 and H_2O.

\text{ Moles of }CaCN_2=\frac{\text{ Mass of }CaCN_2}{\text{ Molar mass of }CaCN_2}=\frac{105.0g}{80.11g/mole}=1.31moles

\text{ Moles of }H_2O=\frac{\text{ Mass of }H_2O}{\text{ Molar mass of }H_2O}=\frac{78.0g}{18g/mole}=4.33moles

Now we have to calculate the limiting and excess reagent.

The balanced chemical reaction is,

CaCN_2+3H_2O\rightarrow CaCO_3+2NH_3

From the balanced reaction we conclude that

As, 1 mole of CaCN_2 react with 3 mole of H_2O

So, 1.31 moles of CaCN_2 react with 1.31\times 3=3.93 moles of H_2O

From this we conclude that, H_2O is an excess reagent because the given moles are greater than the required moles and CaCN_2 is a limiting reagent and it limits the formation of product.

Left moles of excess reactant = 4.33 - 3.93 = 0.4 moles

Now we have to calculate the mass of excess reactant.

\text{ Mass of excess reactant}=\text{ Moles of excess reactant}\times \text{ Molar mass of excess reactant}(H_2O)

\text{ Mass of excess reactant}=(0.4moles)\times (18g/mole)=7.2g

Thus, the leftover amount of excess reagent is, 7.2 grams.

8 0
3 years ago
What fruit does orange fanta taste like??
miv72 [106K]

Answer:

royal

Explanation:

royal is made of orange also

3 0
2 years ago
Read 2 more answers
Select the correct answer.
kondor19780726 [428]

ANSWER: C gases

it has no definite volume and shape and also expands to fill the available volume of the container.

3 0
3 years ago
The magnesium atom in chlorophyll A. is used to pass excited electrons on to pheophytin B. is coupled to the production of ATP C
goblinko [34]

Answer:

B. is coupled to the production of ATP

Explanation:

The magnesium in chlorophyll acts as an activator of enzymes associated with energy metabolism, especially respiratory enzymes and others that act on phosphorylated substrates such as ATP.

7 0
3 years ago
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