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3 years ago

A volume of L is also equal to

Chemistry

1 answer:

Dimas [21]3 years ago

8 0

Answer: One-Thousand of a cubic metre

Explanation:

One lire is the Volume of a cube with 10 cm sides

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What pattern is caused by flammable liquids on the floor

NikAS [45]

The inverted cone, hope it helps .

6 0

3 years ago

Determine the amount of heat energy in joules required to raise the temperature of 7.40g of water from 29.0OC to 46.0 OC.

valina [46]

Answer: The amount of heat energy in joules required to raise the temperature is 526 Joules

Explanation:

The quantity of heat required to raise the temperature of a substance by one degree Celsius is called the specific heat capacity.

$Q=m\times c\times \Delta T$

Q = Heat absorbed = ?

m= mass of substance = 7.40 g

c = specific heat capacity = $4.184J/g^0C$

Initial temperature of the water = $T_i$ = 29.0°C

Final temperature of the water = $T_f$ = 46.0°C

Change in temperature , $\Delta T=T_f-T_i=(46.0-29.0)^0C=17.0^0C$

Putting in the values, we get:

$Q=7.40g\times 4.184J/g^0C\times 17.0^0C$

$Q=526J$

The amount of heat energy in joules required to raise the temperature is 526 Joules

4 0

3 years ago

What volume of nitrogen (n2) would be completely consumed in the reaction with 30.80 g of

Shtirlitz [24]

The answer is 285.33g nitrogen would be completely consumed in the reaction with 30.80 g of hydrogen gas.

A mole is defined as 6.02214076 × 10²³ atoms, molecules, ions, or other chemical units.

Write a balanced equation.

Calculate the moles of H₂ in 30.8 g.

Calculate the moles of N₂ required to react with H₂.

Calculate the mass of N₂.

Calculate the initial mass of N₂.

Start with a balanced equation.

N₂ + 3H₂ --> 2NH₃

Calculate the moles of H₂ in 30.8 g.

n = m/M; where n = moles, m = mass, and M = molar mass.

M(H₂) = 1.008 g/mol

n(H₂) = (30.8 g)/(1.008 g/mol) = 30.56 mol H₂

Calculate the moles of N₂ required to react with 30.56 mol H₂ , using the mole ratio between H₂ and N₂ in the balanced equation.

30.56 mol H₂ × 1 mol N₂/3 mol H₂ = 10.18 mol N₂

Calculate the mass of N₂ in 10.18 mol.

m = n × M

M(N₂) = 2 × 14.007 g/mol N = 28.014 g/mol N₂

m(N₂) = 10.18 mol × 28.014 g/mol = 285.33g N₂

Therefore 285.33g nitrogen would be completely consumed in the reaction with 30.80 g of hydrogen gas.

To know more about mole

brainly.com/question/26416088

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2 years ago

What type of star has an absolute brightness of 1 and a surface temperature around 7,500 °C?

marta [7]

<span>A dim white dwarf star, this is a star with a similar mass to earth. This star has no further fusion reactions at it's core. After this type of star has used up all of it's energy it will become a black dwarf star. Usually they are composed of oxygen and carbon. Sirius a and b are both white dwarf stars that orbit each other.</span>

8 0

3 years ago

Read 2 more answers

C3Hg + 02 → CO2 + H2O

fredd [130]

Answer:

Explanation:

The following equation, which depicts the combustion of propane, is given in this question as follows:

C3H8 + 02 → CO2 + H2O

However, this equation is not yet BALANCED because the number of atoms of each element is not the same on the reactant and product side. To balance the equation, we make use of COEFFICIENT to ensure that the number of atoms of each element on both side correlates.

The balanced equation is as follows:

C3H8 + 502 → 3CO2 + 4H2O

Therefore, the coefficient for water (H2O) after balancing the equation is 4.

8 0

3 years ago