Answer : 0.15 mol of CO2 will remain as excess reactant
(Answer option 4th will be correct)
------------------------------------------------------------------------------------------------------------------------
Solution :
The given
reaction
: 2NaOH (s) + CO2 (g)
Na2CO3 (s) + H2O
(l)
Mole ratio : 2 mol : 1 mol 1 mol : 1 mol
(ratio of coefficients)
Available moles (given mol) : 3.70mol : 2 mol - ; -
From the above mole ratio it is evident that 2 moles of NaOH needs 1 mol of CO2 therefore the moles of CO2 needed to react with the avilable 3.70 moles of NaOH will be
The moles of needed to react with 3.70 moles will be 1.85
The excess of CO2 remains = moles of CO2 available - molesof CO2 needed to react
= 2.00 - 1.85
The excess of CO2 left = 0.15 mol of CO2
Excess of moles of CO2 remains = 0.15 mol
----------------------------------------------------------------------------------------------------------------------------------
From the above calculation it is clear that 0.15 mol of CO2 remains as excess reactant.Therefore all other answer options are wrong.
Sodium hydroxide reacts with carbon dioxide as follows: 2 NaOH(s) + CO2(g) → Na2CO3(s) + H2O(1)...
Sodium hydroxide reacts with carbon dioxide as follows: 2 NaOH(s) + CO2(g) Na2CO3(s) + H2O(1) If 3.70 mol NaOH and 2.00 mol CO2 are allowed to react, how many moles of the excess reactant remains? 0.15 mol CO2 O 0.30 mol NaOH O 1.70 NaOH 1.00 mol CO2 How much energy is required to change the temperature of 1.50 L of water from 25.0 °C to 100.0 °C? The specific heat capacity of water is 4.184 J/g.°C; density H2O =...
Calculate ΔH for the following reaction, CaO(s) + CO2(g) → CaCO3(s) given the thermochemical equations below. 2 Ca(s) + O2(g) → 2 CaO(s) ΔH = -1270.2 kJ C(s) + O2(g) → CO2(g) ΔH = -393.5 kJ 2 Ca(s) + 2 C(s) + 3 O2(g) → 2 CaCO3(s) ΔH = -2413.8 kJ A compound contains C, H and O as the elements. A 20.0 g-sample is comprised of 1.34 g H and also 8.00 g of C. What...
32. Aluminum hydroxide reacts with carbon dioxide as follows: 2 Al(OH)3 (aq) + 3 CO2 (g) → Alz(CO3) (8) + 3 H20 Which is the limiting reactant when 3.0 mol Al(OH)3 and 4.0 mol CO2 are allowed to react? a) Al(OH)3 b) CO2 c) H20 d ) Alz(CO3)3 33. For the above reaction in problem 32, Which is the limiting reactant when 3.0 g of Al(OH)3 and 4.0 g of CO2 are allowed to react? a) Al(OH)3 b) CO2 c)...
Question 19 When 27.0 g of an unknown metal at 88.4 °C is placed in water, the metal is cooled and loses 1300 J of energy. If the final temperature of the water and metal is 23.7 °C, what is the specific heat capacity of the metal? The specific heat capacity of water is 4.184 lg-k. O 0.74 J/g-K O 1.4g. O 0.34 J/g-K O 0.98J/g.K Next Question 20 Calculate AH for the following reaction, CaO(s) + CO2(g) - CaCO3(s)...
4. 2 NaOH (s) + CO2 (g) → NażCO3 (s) + H20 (1) a. Which reagent is the limiting reactant when 1.85 mol NaOH and 1.00 mol CO2 are allowed to react? 704 b. How many moles of Na2CO3 can be produced?
8. Sodium carbonate reacts with hydrobromic acid as follows: Na2CO3(aq) + 2 HBr(aq) -H2O(l) + CO2(g) +2 NaBr(aq) a. (10 points) Write complete ionic and net ionic equations for the reaction above. b. (8 points) Based on the equation above, what volume of carbon dioxide, measured at 815 torr and 455 K, is produced from the complete reaction of 115 mL of 1.25 M hydrobromic acid? Assume excess sodium carbonate.
Sulfuric acid and sodium carbonate react to form carbon dioxide, water, and sodium sulfate as shown in the balanced equation below: H2SO4(aq) + Na2CO3(s) + CO2(g) + H2O(1) + Na2SO4(aq) In the presence of excess sulfuric acid, how many moles of CO2 would be released if you have 12.50 g of Na2CO3(s)? The molar mass of sodium carbonate is 106.0 g/mol, the molar mass of sulfuric acid is 98.08 g/mol, and the molar mass of carbon dioxide is 44.01 g/mol....
Solution Stoichiometry Hydrochloric acid (HCl) reacts with sodium carbonate (Na2CO3), forming sodium chloride (NaCl), water (H2O), and carbon dioxide (CO2). This equation is balanced as written: 2HCl(aq)+Na2CO3(aq)→2NaCl(aq)+H2O(l)+CO2(g) a) What volume of 2.75 M HCl in liters is needed to react completely (with nothing left over) with 0.750 L of 0.300 M Na2CO3? b) A 565-mL sample of unknown HCl solution reacts completely with Na2CO3 to form 10.1 g CO2. What was the concentration of the HCl solution? How do I...
Consider the following unbalanced chemical equation LiOH(s)+CO2(aq)=LiCO3(s)+H2O(l) If 3.89 moles of lithium hydroxide reacts with excess carbon dioxide how many moles of lithium carbonate will be produced
Use the References to access important values if needed for this question. When carbon dioxide reacts with potassium hydroxide, potassium carbonate and water are produced. The balanced equation for this reaction is: CO2(g) + 2KOH(aq) + K,CO3(aq) + H2O(1) If 4 moles of carbon dioxide react, The reaction consumes The reaction produces moles of potassium hydroxide. moles of potassium carbonate and _moles of water