Answer:
2.2 × 10⁻⁴ m
Explanation:
Step 1: Given and required data
- Energy of the wave (E): 9.2 × 10⁻²² J
- Planck's constant (h): 6.63 × 10⁻³⁴ J.s
- Speed of light (c): 3.00 × 10⁸ m/s
Step 2: Calculate the wavelength (λ) of the wave
We will use the following expression.
E = h × c/λ
λ = h × c/E
λ = 6.63 × 10⁻³⁴ J.s × 3.00 × 10⁸ m/s/9.2 × 10⁻²² J
λ = 2.2 × 10⁻⁴ m
Answer:
30.34g (corrected to 4 significant figures).
Explanation:
Take the atomic mass of C=12.0, H=1.0, O=16.0.
no. of moles = mass / molar mass
So, no. of moles of butane reacted = 10 / (12x4 + 1x10)
= 0.172414 mol
Since O2 is in excess and butane is the limiting reagent, the no. of moles of carbon dioxide produced depends on the no. of moles of butane reacted.
From the equation, the mole ratio of butane:Carbon dioxide = 2: 8 = 1: 4,
meaning 1 mole of butane gives 4 moles of CO2.
Using this ratio,
we can deduce that the no. of moles of CO2 produced = 0.172414 x 4
=0.689655 mol
As mass = no. of moles x molar mass
mass of CO2 produced = 0.689655 x (12.0+16.0x2)
=30.34g (corrected to 4 significant figures).
Tritium is an isotope of hydrogen...
For Isotopes number of neutrons are different but electrons and protons are same
Answer:
b
Explanation:
now explanation because that is answer
Answer is: 0,327 g/l.
<span>Ideal gas law: pV = nRT.
</span><span>V - volume, the amount of space occupied by the gas.
</span><span>p - pressure ,1 atm = 760 torr = 760 mmHg.
</span><span>n - amount of substance.
</span>T - temperature, 273 K = 0°<span>C. T = 25 + 273 = 298K.
</span>R - ideal gas constant,<span> R = 0,08206 L</span>·atm/mol·K<span>.
</span>d(He) = M·p ÷ R·T.
d - density.
M - molar mass.
d(He) = 4g/mol · 2atm ÷ 298K · 0,08206 L·atm/mol·K = 0,327 g/l.