How many moles of CaC2 are needed to react completely with 45.0g H2O?

Complete the following equation of nuclear transmutation.

Alekssandra [3086]

Answer:

For the equation of nuclear transmutation, the answer is Option A. 1 0n

Explanation:

Further details on balancing the equation for the reaction presented in the question can be found in the accompanying image.

4 0

1 month ago

A 10.00 g sample of a soluble barium salt is treated with an excess of sodium sulfate to precipitate 11.21 g BaSO4 (M- 233.4). W

eduard [2782]

Answer:

The salt identified is barium chloride.

Explanation:

$BaX_2++Na_2SO_4\rightarrow BaSO_4+2NaX$

The moles of barium sulfate produced are $\frac{11.21 g}{233.38 g/mol}=0.0480 mol$

per the reaction, 1 mole of barium sulfate arises from 1 mole of $BaX_2$ .

Therefore, 0.0480 moles result from:

$\frac{1}{1}\times 0.0480 mol=0.0480 mol$ of $BaX_2$ .

The quantity of $BaX_2$ used amounts to 10.00 g

Moles of $BaX_2$ = \frac{10.00 g}{\text{Molar mass}}[/tex]

$0.0480 mol=\frac{10.00}{\text{Molar mass}}$

The molar mass of $BaX_2$ is 208.33 g/mol

The closest answer to our calculation is $BaCl_2=208.2 g/mol$ .

The correct identification is barium chloride, which has a molar mass of 208.2 g/mol.

8 0

2 months ago

A 250 ml flask contains 3.4 g of neon gas at 45°c. Calculate the pressure of the neon gas inside the flask.

eduard [2782]

The solution to your inquiry yields P = 17.73 atm. Explanation: The volume V is 250 ml, equivalent to 0.25 liters (L), with a mass of 3.4 g and a temperature of 45°C, which converts to 318°K. We utilize the ideal gas law PV = nRT for the calculations.

7 0

1 month ago

A stock solution of Cu2+(aq) was prepared by placing 0.8875 g of solid Cu(NO3)2∙2.5 H2O in a 100.0-mL volumetric flask and dilut

Anarel [2989]

Answer:

3.816 × 10⁻³ M

Explanation:

A stock solution of Cu²⁺(aq) is made by dissolving 0.8875 g of solid Cu(NO₃)₂∙2.5H₂O in a 100.0-mL volumetric flask, and then brought up to volume with water. What is the molarity (in M) of Cu²⁺(aq) in this stock solution?

We can derive the following relations:

The molar mass of Cu(NO₃)₂∙2.5H₂O is 232.59 g/mol.
Each mole of Cu(NO₃)₂∙2.5H₂O yields one mole of Cu²⁺.

The moles of Cu²⁺ present in 0.8875 g of Cu(NO₃)₂∙2.5H₂O are:

$0.8875gCu(NO_{3})_{2}.2.5H_{2}O\times \frac{1molCu(NO_{3})_{2}.2.5H_{2}O}{232.59gCu(NO_{3})_{2}.2.5H_{2}O} \times \frac{1molCu^{2+} }{1molCu(NO_{3})_{2}.2.5H_{2}O} =3.816\times10^{-3} molCu^{2+}$

The molarity of Cu²⁺ is:

$\frac{3.816\times10^{-3} mol}{100.0 \times10^{-3}L} =3.816\times10^{-2}M$

4 0

2 months ago

A careless student forgets to label one of their reagent containers. They know it contains one of the following solutions: 0.1 M

castortr0y [3046]

Sagot:

0.1 M NaCl

Paliwanag:

Ang tanong na ito ay nagpapaalala sa atin ng mga patakaran sa solubility. Alalahanin natin na ang lahat ng chlorides ay natutunaw maliban sa mga ng lead, mercury II at silver na hindi natutunaw sa tubig.

Ang sumusunod na reaksyon ay mangyayari na humahantong sa pagbuo ng isang precipitate;

Pb(NO3)2(aq) + 2NaCl(aq) -------> 2NaNO3(aq) + PbCl2(s)

Ang puting precipitate na nabuo ay PbCl2.

4 0

2 months ago