Answer:
The pressure equilibrium constant (Kp) = (P O₂)³/(P CO₂)²(P H₂O)⁴.
Explanation:
<em>2CO₂ (g) + 4H₂O (g) → 2CH₃OH (l) + 3O₂ (g).</em>
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The pressure equilibrium constant (Kp) = the product of the pressure of the products side components / the product of the pressure of the reactantss side components.
each one is raised to a power equal to its coefficient.
<em>∴ The pressure equilibrium constant (Kp) = (P O₂)³/(P CO₂)²(P H₂O)⁴.</em>
I'm not sure, but I believe the correct answer is C.
Answer:
4Na + O₂ → 2Na₂O
6.82g
Explanation:
The combustion of sodium involves combining the element with oxygen gas:
4Na + O₂ → 2Na₂O
We have been given 5g of Na.
The balanced reaction equation is given as shown above. This reaction is also a synthesis or combination reaction.
b. Maximum amount of product that can be obtained.
Sodium is the limiting reactant and it will determine the amount of product that can be formed.
To solve this, we find the number of moles of the given sodium.
Mass of given sodium = 5g
Molar mass of Na = 23g/mol
Number of moles of Na =
Insert the parameters and solve;
Number of moles of Na =
= 0.217moles
From the balanced reaction equation:
4 moles of Na will produce 2 moles of Na₂O
0.217 moles of Na will produce
= 0.11mole of Na₂O
So;
Mass of Na₂O = number of moles x molar mass
Molar mass of Na₂O = 2(23) + 16 = 62g/mol
Mass of Na₂O = 0.11 x 62 = 6.82g
Answer:
This metal could be lead
Specific heat = 0.0308 cal/g°C
Explanation:
Step 1: Data given
The metal was heated to 115.0°C
in a calorimeter where it cooled to 32.6°C.
Mass of the metal = 25.0 grams
Heat released = 63.5 cal
Step 2: Calculate the specific heat of the metal
Q = m*c*ΔT
⇒with Q = the heat released = 63.5 cal
⇒with m = the mass of the metal = 25.0 grams
⇒with ΔT = the change of temperature = T2 - T1 = 32.6 °C - 115.0°C = -82.4 °C
⇒ c = the specific heat = TO BE DETERMINED
63.5 = 25.0 * c * 82.4
C = 0.0308 cal/g°C
This metal could be lead
The electrons used in fireworks are in excited state.