Molar mass of SnO_2:-
1 mol of SnO_2 produces 2mol of water
- 0.5mol of SnO_2 will produce 0.5(2)=1mol of water
Answer:
The given substance is cast iron.
Explanation:
Given data:
Mass of substance = 50 g
Heat absorbed = 23000 J
Initial temperature = 250°C
Final temperature = 1250°C
Which metal is this = ?
Solution:
Specific heat capacity:
It is the amount of heat required to raise the temperature of one gram of substance by one degree.
Formula:
Q = m.c. ΔT
Q = amount of heat absorbed or released
m = mass of given substance
c = specific heat capacity of substance
ΔT = change in temperature
ΔT = 1250°C - 250°C
ΔT = 1000°C
23000 j = 50 g ×c ×1000 °C
23000 J = 50,000 g. °C×c
c = 23000 J /50,000 g. °C
c = 0.46 J/g.°C
The given substance is cast iron.
Answer:
substance
Explanation:
A mixture is when two or more <u>different</u> atoms/molecules are together, but not joined.
A substance is when the <u>same </u>atom/molecule is in a group together.
In this example, it is a substance because it is comprised of the same molecule not joined all together. If you wanted a mixture, other colored atoms/molecule (e.g. add green atoms) would change it to this property.
Answer:
16 mg of water can be produced by 7.1×10⁻³ g of CH₄
Explanation:
This is the reaction:
CH₄ + 2O₂ → CO₂ + 2H₂O
In a combustion, oxgen is a reactant with another compound, and the products are always water and carbon dioxide
1 mol of methane can produce 2 moles of water. Ratio is 1:2
If we convert the mass to moles → 7.1×10⁻³ g . 1 mol/ 16g = 4.43×10⁻⁴ mol
In this reaction I would produce the double of moles I have from methane, so If I have 4.43×10⁻⁴ moles of methane I would produce 8.87×10⁻⁴ moles of water.
What mass of water, corresponds to 8.87×10⁻⁴ moles?
8.87×10⁻⁴ mol . 18g / 1mol = 0.016 g which is actually the same as 16 mg
the control rods absorb extra neutrons keeping them from causing to many uranium atoms to split to quickly.
