What is the charge of this atom? 65 protons 60 electrons A)-5 B)+5 C)0

What does amoeba use to move and ingest prey?

melomori [17]

The cytoplasm slides and forms a pseudopodium in front to move the cell forwards.

7 0

2 years ago

A 1.00 g sample of a metal X (that is known to form X ions in solution) was added to 127.9 mL of 0.5000 M sulfuric acid. After a

Semenov [28]

Answer: The metal having molar mass equal to 26.95 g/mol is Aluminium

Explanation:

To calculate the number of moles for given molarity, we use the equation:

$\text{Molarity of the solution}=\frac{\text{Moles of solute}}{\text{Volume of solution (in L)}}$ .....(1)

Molarity of NaOH solution = 0.5000 M

Volume of solution = 0.03340 L

Putting values in equation 1, we get:

$0.5000M=\frac{\text{Moles of NaOH}}{0.03340L}\\\\\text{Moles of NaOH}=(0.5000mol/L\times 0.03340L)=0.01670mol$

The chemical equation for the reaction of NaOH and sulfuric acid follows:

$2NaOH+H_2SO_4\rightarrow Na_2SO_4+H_2O$

By Stoichiometry of the reaction:

2 moles of NaOH reacts with 1 mole of sulfuric acid

So, 0.01670 moles of NaOH will react with = $\frac{1}{2}\times 0.01670=0.00835mol$ of sulfuric acid

Excess moles of sulfuric acid = 0.00835 moles

Calculating the moles of sulfuric acid by using equation 1, we get:

Molarity of sulfuric acid solution = 0.5000 M

Volume of solution = 127.9 mL = 0.1279 L (Conversion factor: 1 L = 1000 mL)

Putting values in equation 1, we get:

$0.5000M=\frac{\text{Moles of }H_2SO_4}{0.1279L}\\\\\text{Moles of }H_2SO_4=(0.5000mol/L\times 0.1279L)=0.06395mol$

Number of moles of sulfuric acid reacted = 0.06395 - 0.00835 = 0.0556 moles

The chemical equation for the reaction of metal (forming $M^{3+}$ ion) and sulfuric acid follows:

$2X+3H_2SO_4\rightarrow X_2(SO_4)_3+3H_2$

By Stoichiometry of the reaction:

3 moles of sulfuric acid reacts with 2 moles of metal

So, 0.0556 moles of sulfuric acid will react with = $\frac{2}{3}\times 0.0556=0.0371mol$ of metal

To calculate the molar mass of metal for given number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

Mass of metal = 1.00 g

Moles of metal = 0.0371 moles

Putting values in above equation, we get:

$0.0371mol=\frac{1.00g}{\text{Molar mass of metal}}\\\\\text{Molar mass of metal}=\frac{1.00g}{0.0371mol}=26.95g/mol$

Hence, the metal having molar mass equal to 26.95 g/mol is Aluminium

6 0

3 years ago

Ill give u brainliest help asap

Anna007 [38]

I think its A. it cant be C or D b/c we are measuring the distance between Earth and Saturn, not the speed.

7 0

2 years ago

What is the mass of 6.12 moles of arsenic (As)?

Alecsey [184]

The answer is D. 459 g As

5 0

3 years ago

Read 2 more answers

Which of the following is the correctly balanced chemical equation for the reaction of Ca(OH)2 and HNO3?

sattari [20]

Explanation:

The reaction between calcium hydroxide and nitric acid is as follows.

$Ca(OH)_{2} + HNO_{3} \rightarrow Ca(NO_{3})_{2} + H_{2}O$

Number of reactant atoms are as follows.

Ca = 1
O = 4
H = 3
N = 1

Number of product atoms are as follows.

Ca = 1
O = 4
H = 2
N = 3

To balance the given chemical equation, multiply $HNO_{3}$ by 2 on reactant side and multiply $H_{2}O$ by 2 on the product side.

Therefore, the balanced chemical equation will be as follows.

$Ca(OH)_{2} + 2HNO_{3} \rightarrow Ca(NO_{3})_{2} + 2H_{2}O$

4 0

3 years ago