16. Relevant information is knowledge that relates to the question. True or false

Write balanced molecular equation for the reaction between nitric acid and calcium hydroxide. Express your answer as a chemical

Alisiya [41]

Answer:

2HNO3 + Ca(OH)2 ===> Ca(NO3)2 + 2H2O

Explanation:

This a neutralisation reaction. The first thing to note is that this type of reaction forms salt and water.

Note that the formula of water is H2O. So write this at the right hand side.

==> H2O

Next note that the salt should contain the acid radical (NO3) and the metallic part of the base (Ca) written well following the rule for writing chemical equation; thus

==> Ca(NO3)2 + H2O

The next step is to write the reactants at the right hand side of the equation;

HNO3 + Ca(OH)2 ==> Ca(NO3)2 + H2O

The final step is to count the number of atoms in each side of the equation to make sure they are equal and balanced.

In the above equation, H atoms are three at the left hand side add 2 to to H- containig compound on both side as to balance up. Thus

2HNO3 + Ca(OH)2 ===> Ca(NO3)2 + 2H2O

The equation 2HNO3 + Ca(OH)2 ===> Ca(NO3)2 + 2H2O is balance.

4 0

3 years ago

Covert 1.57 x 10^14 nm= ___m

LekaFEV [45]

Answer:

1.57 x 10⁷m

Explanation:

Given quantity is;

1.57 x 10¹⁴nm

Now;

1 nm = 10⁻⁹

So, let us convert this given quantity;

1 nm = 10⁻⁹

1.57 x 10¹⁴nm will give 1.57 x 10¹⁴ x 10⁻⁹ = 1.57 x 10⁷m

7 0

3 years ago

A substance has a mass of 360 g and a volume of 7.5 cm3. What is its density?

a_sh-v [17]

D = g / cm³

Density = mass / volume

D = 360 g / 7.5 cm³

D = 48 g/cm³

answer D

hope this helps!

7 0

3 years ago

Dihydrogen dioxide decomposes into water and oxygen gas. Calculate the amounts requested if 1.34 moles of dihydrogen dioxide rea

a_sh-v [17]

Answers:

a. Moles of oxygen formed: 0.670 mol

b. Moles of water formed: 1.34 mol

c. Mass of water formed: 24.1 g

d. Mass of oxygen formed: 21.4 g

Explanation:

Dihdyrogen dioxide is the chemical name for a compound made of two hydrogen atoms and two oxide atoms, i.e. H₂O₂, which is also known as hydrogen peroxide or oxygenated water.

The decomposition reaction of dihydrogen dioxide into water and oxygen gas is represented by the balanced chemical equation:

$2H_2O_2(l)\rightarrow 2H_2O(l)+O_2(g)$

The mole ratios derived from that balanced chemical equation are:

2 mol H₂O₂ : 2 mol H₂O : 1 mol O₂

a. Moles of oxygen formed

Set the proportion using the theoretical mole ratio of H₂O₂ to O₂ and the amount of moles of dyhydrogen dioxide that react:

$2\text{ mol }H_2O_2/1\text{ mol }O_2=1.34\text{ mol }H_2O_2/x$

When you solve for x, you get:

x = 1.34 mol H₂O₂ × 1 mol O₂ / 2 mol H₂O₂ = 0.670 mol O₂

b. Moles of water formed

Set the proportion using the theoretical mole ratio of H₂O₂ to H₂O and the amount of moles of dyhydrogen dioxide that react:

$2\text{ mol }H_2O_2/2\text{ mol }H_2O=1.34\text{ mol }H_2O_2/x$

When you solve for x, you get:

x = 1.34 mol H₂O₂ × 2 mol H₂O / 2 mol H₂O₂ = 1.34 mol H₂O

c. Mass of water formed

Using the number of moles of water calculated in the part b., you calculate the mass of water formed, in grams, using the molar mass of water:

Molar mass of water = 18.015 g/mol

Number of moles = mass in grams / molar mass

⇒ mass in grams = number of moles × molar mass

⇒ mass in grams = 1.34 mol × 18.015 g/mol = 24.1 g

d. Mass of oxygen formed

Using the number of moles of oxygen determined in the part a., you calculate the mass in grams using the molar mass of O₂.

Molar mass of O₂ = 32.00 g/mol

mass = molar mass × number of moles

mass = 32.00 g/mol × 0.670 mol = 21.4 g.

5 0

3 years ago

Rank the four gases (air, exhaled air, gas produced from the decomposition of H2O2, gas from decomposition of NaHCO3) in order o

ddd [48]

air = 70 % N2 exhaled air =70%N2 + some less O2 compared to only air 2H2O2=2H2O+O2 NaHCO3=2NaHCO3 → Na2CO3 + H2O + CO2 = No O2 gas from decomposition ssoooo NaHCO3 <exhaled air <air <H2O2

SO sorry for the long wait, hope I helped.

4 0

3 years ago