What is the name for B2(SO4)3

Find the mass of 1.59 mol of NH3

xxMikexx [17]

Answer:

27.03 grams

Explanation:

moles (n) = mass(m)/Molar mass(M)

moles = 1.59

mass = ?

N = 14, H = 1

M(NH3) = 14 + 3(1) = 17

Substitute the values into the equation:

nM = m

∴ m = 1.59 × 17 = 27.03

5 0

3 years ago

Does anyone know the answer to this chemistry question?!?

Pepsi [2]

Answer:

Mass of HCl = 73 g

Explanation:

Given data:

Mass of hydrogen = 2 g

Mass of HCl = ?

Solution:

First of all we will write the balance chemical equation:

H₂ + Cl₂ → 2HCl

Number of moles of hydrogen = 2 g/ 2g/mol

Number of moles of hydrogen = 1 mol

Form balanced chemical equation compare the moles hydrogen with HCl.

H₂ : HCl

1 : 2

Mass of HCl:

Mass of HCl = number of moles × molar mass

Mass of HCl = 2 mol × 36.5 g/mol

Mass of HCl = 73 g

7 0

4 years ago

A chemical supply company sells a concentrated solution of aqueous h2so4 (molar mass 98 g mol−1 ) that is 50. percent h2so4 by m

trapecia [35]

Answer is: the molarity of the sulfuric acid is 7.14 M.
ω(H₂SO₄) = 50% ÷ 100% = 0.5.
d(H₂SO₄) = 1.4 g/mL.
V(H₂SO₄) = 100 mL ÷ 1000 mL/L = 0.1 L..
mr(H₂SO₄) = d(H₂SO₄) · V(H₂SO₄).
mr(H₂SO₄) = 1.4 g/mL · 100 mL.
mr(H₂SO₄) = 140 g.
m(H₂SO₄) = ω(H₂SO₄) · mr(H₂SO₄).
m(H₂SO₄) = 0.5 · 140 g.
m(H₂SO₄) = 70 g.
n(H₂SO₄) = m(H₂SO₄) ÷ M(H₂SO₄).
n(H₂SO₄) = 70 g ÷ 98 g/mol.
n(H₂SO₄) = 0.714 mol.
c(H₂SO₄) = n(H₂SO₄) ÷ V(H₂SO₄).
c(H₂SO₄) = 0.714 mol ÷ 0.1 L.
C(H₂SO₄) = 7.14 M.

8 0

3 years ago

A 5.90-g sample of an unknown compound containing only C, H, and O combusts in an oxygen rich environment. When the products hav

Over [174]

Answer:

The empirical formula is C4H8O

The molecular formula is C8H16O2

Explanation:

Step 1: Data given

Mass of the unknown sample = 5.90 grams

Temperature = 20.0 °C

PRessure = 1 bar

Volume CO2 = 7.98 L

Volume of H2O = 5.91 mL = 0.00591 L

Density of water at 20.0 °C = 0.998 g/mL

Step 2: Calculate moles CO2

p*V= n*R*T

⇒ with p = the pressure = 1 bar = 0.986923 atm

⇒ with V = the volume of CO2 = 7.98 L

⇒ with n = the number of moles CO2 = TO BE DETERMINED

⇒ with R = The gas constant = 0.08206 L*atm/K*mol

⇒ with T = the temperature = 20.0 °C = 293 Kelvin

n = (p*V)/(R*T)

n = (0.986923*7.98)/(0.08206*293)

n = 0.3276 moles

Step 3: Calculate mass water

Mass water = volume * density

Mass water = 5.91 mL * 0.998 g/mL

Mass water = 5.89818 grams

Step 4: Calculate moles H2O

Moles H2O = 5.89818 grams / 18.02 g/mol

Moles H2O = 0.3273 moles

Step 5: Calculate moles of hydrogen

For 1 mol H2O we have 2 moles of hydrogen

For 0.3273 moles H2O we have 2*0.3273 moles = 0.6546 moles

Step 6: Calculate moles of carbon

1 mol CO2 has 1 mol C

0.3276 moles moles CO2 has 0.3276 moles C

Step 7: Calculate mass C

Mass C = 0.3276 moles * 12.0 g/mol

Mass C = 3.93 grams

Step 8: calculate mass of oxygen

Mass of O = mass of sample - (mass of C + mass of H)

Mass O = 5.90 grams - (3.93 +0.661 )

Mass O = 1.309 grams

Step 9: Calculate moles O

Moles O = 1.309 grams / 16.0 g/mol

Moles O = 0.0818 moles

Step 10: Calculate mol ratio

We divide by the smallest amount of moles

C: 0.3276 / 0.0818 = 4

H: 0.6546 / 0.0818 = 8

O: 0.0818 / 0.0818 = 1

The empirical formula is C4H8O

If the molar mass is 144.2

The molecular formula is C8H16O2

8 0

4 years ago

What is the kinetic product obtained from the addition of 1 equivalent of HBr to 1,3-butadiene?

pentagon [3]

Answer:

From the addition of 1 equivalent of HBr to 1,3-butadiene, 3-bromo-1-butene is obtained as a product.

7 0

4 years ago